SOLUTIONS
SECTION 12.1
1. Review mixtures, then give a definition and four examples of each:
DEFINITION EXAMPLES
HOMOGENEOUS MIXTURE
HETEROGENEOUS MIXTURE
2. Define the following terms: SOLUTION
SOLVENT
SOLUTE
SOLUBLE
3. Explain the description of a solution as a “particle-by-particle mixture:”
4. List five substances that are soluble in water:
5. List five substances that are insoluble in water:
6. Many people feel that “solution” specifically refers to a solid dissolved in a liquid. Is this correct? EXPLAIN: 7. Describe what an alloy is:
8. Define the following: SUSPENSION
COLLOID
GEL
FOAM
(LIQUID) EMULSION
TYNDALL EFFECT
Complete the following table of characteristics of solutions, colloids, and suspensions:
SOLUTIONS COLLOIDS SUSPENSIONS SOLUTIONS, pp 3 and 4
SECTION 12.1 and SECTION 13.1
1. DEFINE: ELECTROLYTE
NONELECTROLYTE
2. Give four examples of nonelectrolytes:
3. Electrolytes are ______compounds, or highly ______covalent compounds.
4. Give four examples of electrolytes:
5. Define: DISSOCIATION
IONIZATION
6. Please write equations to show dissolving of the following substances (in water). + - example: NaCl(s) -- Na (aq) + Cl (aq)
C6H12O6
Ca3(PO4)2
NaNO3
O2
HINTS: Did you consider whether or not the substance is an electrolyte? Did you write a BALANCED equation? 7. DEFINE: STRONG ELECTROLYTE
WEAK ELECTROLYTE
8. Please write equations to show dissolving of the following substances (in water). (See page 860)
Barium carbonate
Sodium hydroxide
Potassium sulfate
Manganese(II) phosphate
HINTS: Did you consider whether the substance is a strong or weak electrolyte? Did you write a BALANCED equation?
9. Please write TOTAL and NET ionic equations to show the following reactions: (See page 860)
Solutions of potassium hydroxide and iron(II) chloride
Solutions of copper(II) acetate and sodium phosphate SOLUTIONS, pp 5 and 6
1. List three methods of increasing the RATE at which a substance dissolves:
2. Which of these actually increases the AMOUNT of substance that dissolves?
3. Explain the phrase "like dissolves like."
4. Define SOLUBILITY:
ANSWER the following questions, using pages 414 and 410: o 5. What is the solubility of C12H22O11 at 10 C? ______o 6. What is the solubility of NaNO3 at 70 C? ______o 7. What is the solubility of CO2 at 20 C? ______8. What is the solubility of KCl at 90oC? ______
9. ______g of KI could dissolve in 100g of water at 10oC. o 10. ______g of KNO3 could dissolve in 100g of water at 70 C. 11. ______g of KI could dissolve in 200g of water at 40oC. o 12. ______g of KNO3 could dissolve in 50g of water at 20 C. 13. Define: SATURATED SOLUTION
14. Explain how to make a saturated solution: 15. Define: UNSATURATED SOLUTION
SUPERSATURATED SOLUTION
16. Explain how to make a SUPERSATURATED solution:
#17-20: IDENTIFY the following solutions as saturated, unsaturated, or supersaturated: (see pp 414, 410) o ______17. 31.6g KNO3 in 100g of water at 20 C. o ______18. 31.6g KNO3 in 200g of water at 20 C. o ______19. 111g Ba(OH)2 in 100g of water at 80 C. o ______20. .180g Ca(OH)2 in 100g of water at 30 C. #21 - 24: IDENTIFY the following solutions as saturated, unsaturated, or supersaturated: o ______21. 22g KNO3 in 100g of water at 20 C. o ______22. 35g KNO3 in 70g of water at 20 C. o ______23. 88g Ba(OH)2 in 100g of water at 80 C. o ______24. .300g Ca(OH)2 in 100g of water at 30 C. 25. The solubility of most solids ______as temperature increases.
26. Which solids have solubilities that DECREASE as temperature increases? ______
27. How can the solubility of a gas be increased?
28. Brook trout have a high demand for oxygen. Where are brook trout found? Why? Read "Weighting In The Wings" in the December 1997 ChemMatters and answer the following questions:
1. In what ways can icing affect planes?
______
______
______
2. Is icing DURING flight a problem? _____ Explain:
3. What is supercooled water?
4. What methods are available to deal with in-flight icing?
A.______
B.______
C.______
5. Ethylene glycol is an effective deicer, but efforts are underway to use less ethylene glycol. Why?
6. What method is being employed in Munich and Denver to decrease the amount of ethylene glycol entering the environment?
7. Describe the major effect of ethylene glycol on the environment: Read the article "Dissolving Household Chores" in the December 1997 ChemMatters and answer the following:
1. Chemist Bob Black sought a new way to deal with the problem of:
2. Bob identified substances that clean without mechanical action ("SCRUBBING") and that:
A.______
B.______
3. "Bob chose a ______to lift the deposits off of the shower wall." More technically, the compound is an______ether of a long chain alcohol.
4. Define hydrophobic:
5. What two elements are involved in the bonding at the hydrophobic end of this molecule? _____ and _____ Compute the electronegativity difference of these two elements.______What type of bonding exists at this end of the molecule?______
6. Define hydrophilic:
7. At the hydrophilic end of this molecule we see bonds of two types. Compute the EN difference for C-O bonds ______and for O-H bonds _____. What type of bonding exists at this end of the molecule?______
8. What type of bonding exists in water molecules?______
9. What is meant by the phrase "like dissolves like"?
10. Circle the following substances you would expect to dissolve in water
SI2 NH3 H2 CH4 NCl3 HCl PCl3 H2S CO2 I2O
11. Read the extra sections, particularly the one titled "Wetting Agents"
12. Draw the structure of isopropyl alcohol, and label the portions of the molecule that are hydrophilic (water- attracting) and hydrophobic (oil-attracting).
13. Can you think of any other possible uses of molecules that have both hydrophobic and hydrophilic ends? SOLUBILITY LAB: SOLUBILTY OF ______
PURPOSE: The purpose of this lab is to determine the solubility of a given substance at various temperatures. This data will then be used to create a solubility curve for the given substance.
PRELAB: 1. Write an equation to show dissolving (at equilibrium) of the solute in water:
2. Define SOLUBILITY:
3. How can we ensure that the solution is saturated?
4. The solubility of most solids ______as temperature increases.
PROCEDURE:
1. Mass a petri or evaporating dish. ______2. Form a heated, saturated solution of the solute. 3. Record the temperature of the saturated solution. ______4. Carefully pour a small quantity of the solution into the dish. 5. Carefully remass the dish. ______6. Set the dish aside (overnight) so the water can evaporate. 7. After all water has evaporated, remass the dish. ______8. Clean up, as instructed.
POST-LAB: 1. Do the necessary calculations and complete the table below. 2. Create a graph (solubility curve) of the data.
mass of mass of mass of solute water Temp. empty dish and dish and mass mass SOLUBILITY o ( C) dish (g) solution (g) solute (g) (g) (g) (g/100gH2O)
______
______
______
______
______
______
______
______
______CHEMISTRY LAB -- ENTHALPY OF SOLUTION
OBJECTIVE: The purpose of this lab is to determine the enthalpy of solution (in kJ/mol) of various compounds.
WARNINGS: Safety glasses must be worn the entire time. NaOH is extremely corrosive and can cause severe burns or eye damage. NH4NO3 must also be treated with caution. Dispose of all chemicals as instructed.
PROCEDURE: 1. Measure and record the mass of a plastic foam cup (calorimeter). 2. Add approximately 1.0 g NaOH pellets to the cup. 3. Mass the cup and NaOH. 4. Measure approximately 50 ml of distilled water in a graduated cylinder and record the volume and temperature. 5. Add the water to the NaOH in the cup. Stir the mixture with a glass stirring rod and record the highest temperature reached.
Mass of cup ______Water volume______
Mass of cup and solute ______Original water temp. ______
Final water temp. ______
ENTHALPY OF SOLUTION OF NH4NO3:
Repeat the procedure above to find the enthalpy of solution of NH4NO3, recording all important data below. Use approximately 5.0 g NH4NO3.
Mass of cup ______Water volume______
Mass of cup and solute ______Original water temp. ______
Final water temp. ______
POSTLAB: Write ONLY THE CALCULATIONS AND CONCLUSIONS sections of a lab report, with the following considerations: 1. Include all calculations for YOUR data, for both compounds. Use three step format! 2. Discuss your results in conclusions. 3. Include a good discussion of possible sources of error and their effects. Do NOT include such silly things as "The balance was off." or "I read the thermometer wrong." 4. Calculate the enthalpy of solution of compound X if it has a formula mass of 90.25g and 2.44g causes 100.0 ml of water to go from 22.7oC to 26.1oC. HEAT OF SOLUTION PROBLEMS , p.1 NAME______
1. Determine the heat of solution of Spartonous (M = 100.0 g/mol) if 2.0g causes 50g of water to go from 22.3 oC to 28.3 oC.
2. Determine the heat of solution of Schoolium (M = 80.0 g/mol) if 4.0g causes 50g of water to go from 22.3 oC to 17.3 oC.
o 3A. Determine the mass of KClO3 that would cause a temperature change of 5.7 C for 250g of water.
3B. Will temperature rise or fall? Explain how you know: HEAT OF SOLUTION PROBLEMS , p.2 NAME______
1) 2.70 g of potassium hydroxide was added to 64.7g of water at 19.6oC. What is the final temperature of the water?
2) Hydrogen chloride was added to 200ml of water and the temperature went from 19.0oC to 25.7oC. What mass of hydrogen chloride was added?
3) You are designing an instant ice pack, using water and an appropriate solute. Choose an appropriate solute and write it in the blank at right: ______Calculate the mass of this solute needed to cool 300g of water from 25oC to 5oC.
4) What other factors might affect your choice of a solute to actually use in an instant ice pack? Explain. HEAT OF SOLUTION PROBLEMS , p.3 NAME______
1. 4.2g of compound X (formula mass is 110 g/mol) was added to 89.3g of water. o o The temperature of the water dropped from 23.4 C to 20.8 C. Compute ∆Hsol for compound X:
2. Was this (the dissolving of X in water) an endothermic or exothermic process? Explain how you can tell:
3. Why does X dissolve? (What is the "driving force" for this particular change?) Explain:
4. A solution equilibrium was established: X(s) ↔ X(aq) . If temperature is increased, what will happen to the solubility of X? Explain, with reference to Le Chatelier's Principle: CHEMISTRY LAB -- ENTHALPY OF REACTION
OBJECTIVE: The purpose of this lab is to determine the enthalpy of reaction (in kJ/mol) of the reaction of hydrochloric acid and potassium hydroxide.
WARNINGS: Safety glasses must be worn the entire time. KOH is extremely caustic and can cause severe burns or eye damage. Obviously, HCl must also be treated with caution. Dispose of all chemicals as instructed.
PROCEDURE: 1. Measure and record the mass of a plastic foam cup (calorimeter). 2. Add approximately 1.0 g KOH pellets to the cup. 3. Mass the cup and KOH. 4. Measure approx. 50 ml of 3M HCl in a graduated cylinder and record the volume and temperature. 5. Add the acid to the NaOH in the cup. Stir the mixture with a glass stirring rod and record the highest temperature reached.
______
Mass of cup ______Water volume______
Mass of cup and solute ______Original water temp. ______
Final water temp. ______
Here, record your value for the heat of solution of KOH, from the previous lab: ______
______
1. What TWO processes caused the temperature to rise?
CALCULATIONS:
1. Calculate the heat change of the water:
2. Indicate the heat change of the KOH: ______3. Calculate the moles of KOH:
4. Calculate the heat change PER MOLE of KOH:
5. This value (from prior calc.) is for BOTH PROCESSES: ______List both processes:
A.
B.
6. Recall your value for Hsol of KOH: ______
7. Find the difference of these values: ______This is the heat change caused by the second process, which was the actual reaction of KOH and HCl.
8. So, the enthalpy of ______of HCl and KOH is ______.
9. Write the equation for the chemical reaction of KOH and HCl, including the value from above, which is the enthalpy of reaction.
Follow-up: 1. Write the equation for the reaction of solutions of sodium hydroxide and nitric acid:
2. Write the equation for the reaction of solutions of sodium hydroxide and ferric chloride: ENTHALPY, ENTROPY, AND FREE ENERGY
So far we have been talking about enthalpy (heat, energy: "Things go to lower energy.") as a "driving force" of reactions and processes. Here, we will see that there is another driving force that must be considered.
1. Define ENTHALPY:
2. We know that processes tend to go from ______energy to _____ energy.
3. Label each of the following as "favored" or "not favored":
ENDOTHERMIC PROCESSES (delta H is positive) ______
EXOTHERMIC PROCESSES (delta H is negative) ______
4. If energy change was the ONLY consideration, we would say that
______processes CANNOT ever occur (are never spontaneous).
5. Read pages 546-548.
6. Define SPONTANEOUS:
7. What are the TWO factors that must be considered when determining if a reaction "will go" (is spontaneous)? ______, ______
8. Define ENTROPY
9. Next to each, indicate the type of change that would indicate a process is favored:
quantity “increase” or “decrease” mathematical sign
ENTHALPY
ENTROPY
9. Now fill in the table below with the four possible combinations and indicate "always." "never," or "depends on temperature" in the last column:
SIGN OF THE SIGN OF THE ENTHALPY CHANGE ENTROPY CHANGE SPONTANEITY ENTHALPY, ENTROPY, AND FREE ENERGY, p.2
We will look at a few processes and describe the enthalpy and entropy changes, then see if we can determine the spontaneity of the process (similar to the prior question).
1. MELTING OF A SNOWFLAKE
A. Describe the change of enthalpy (heat, "energy") as "positive" or "negative," and explain how you know this:
B. This______enthalpy change indicates the process ______favored.
C. Describe the entropy change and explain:
D. This______entropy change indicates the process ______favored.
E. Therefore, is the process spontaneous (favored)? The three possibilities are: "always", "never", or "depends on T".
2. DISSOLVING OF NaOH IN WATER (see page 416)
A. Describe the change of enthalpy (heat, "energy") as "positive" or "negative," and explain how you know this:
B. This______enthalpy change indicates the process ______favored.
C. Describe the entropy change and explain:
D. This______entropy change indicates the process ______favored.
E. Therefore, is the process spontaneous (favored)? The three possibilities are: "always", "never", or "depends on T". ENTHALPY, ENTROPY, AND FREE ENERGY, p.3
1. Read pp 548-550 to get "the rest of the story."
2. Define "spontaneous:"
3. What is the ONE criterion that indicates if a reaction/process is spontaneous?
4. State the equation for free energy change: ______
5. We will examine two changes in detail, numbers 6 and 7 below.
6. For the process: LiCl(s) -- LiCl(aq) ∆Hsol = -35.0 kJ/mol
6A. The enthalpy change of ______indicates the process ______favored.
6B. The entropy change of +9.80 J/mol•Co indicates the process ______favored.
6C. We would expect the process to be spontaneous: always never that depends on temperature
6D. Calculate ∆G for this process at 25oC.
7. For the process: H2O(l) -- H2O(g)
7A. The enthalpy change of +44.014 kJ/mol indicates the process ______favored.
7B. The entropy change of +118.78 J/mol•Co indicates the process ______favored.
7C. We would expect the process to be spontaneous: always never that depends on temperature
7D. Calculate ∆G for this process at 25oC.
7E. At what temperature would ∆G = 0?
7F. What is special about this temperature? ______Recall our definition of boiling point: The temperature at which the ______vapor pressure is equivalent to the external temperature. CHEMISTRY PRETEST -- SOLUTIONS NAME:______
1. Make a vocab list of appropriate terms and define.
2. To cause a solid to dissolve more quickly, one can:
A.______
B.______
C.______
3. List four substances that are soluble in water, and four that are insoluble in water: SOLUBLE IN WATER INSOLUBLE IN WATER
A.______A.______
B.______B.______
C.______C.______
D.______D.______
4. The surrounding of solute particles by solvent particles is called ______.
5. The surrounding of solute particles by WATER particles is called ______.
6. Soap can be used to dissolve grease in water because soap molecules have a ______end that attaches to grease molecules and a ______end that attaches to water molecules.
PROBLEMS:
7. 3.00 moles of KNO3 was dissolved 8. 1.10g CO2 was dissolved in in water to make 1.50 liters of water to make 2.00 liters of solution. Compute the molarity solution. Compute the molarity of this solution: of this solution:
9. A chemist measures out 250 ml of .600M HCl. How many moles of HCl are in this solution (250 ml of .600M HCl)?
10. A chemist wants to obtain .045 moles of CaCl2. What volume of .180 M CaCl2 must she use? 11. A mixture was tested and found to contain 40.0g MgBr2 and 90.1g H2O. What was the mass percent of CaBr2 in this solution?
12. 7.8g of BaI2 was dissolved in 100 ml of water. The temperature of the water o o went from 22.1 C to 24.2 C. Find the enthalpy of solution of BaI2. The specific heat of water is 4.184 J/(g*oC).
13. Compound X has a molar mass of 166.1 g/mol and a heat of solution of +35.2 kJ/mol. Determine the mass of X needed to cause 75.3g of water to change temperature by 3.4 degrees C. What is the final temperature?
14. What mass of sodium hydroxide would be needed to neutralize 452 ml of .250 M sulfuric acid? Include balanced equation.
15. Compound Z has a molar mass of 104.8 g/mol. Determine the heat of solution of Z if 4.55g causes 72.47g of water to go from 24.1oC to 18.9oC. MOLARITY (M) and molality (m)
1. Define and give abbreviations for each:
molarity (__):
molality (__):
For each of the following problems you must:
A. FIRST determine if the data provided allows you to calculate molarity or molality. Indicate with the appropriate abbreviation on the blank to the left of each problem.
B. Calculate the approprate concentration.
______2. 5.44g of glucose was dissolved in enough water to make exactly 250ml of solution:
______3. .988g of sodium phosphate was dissolved in 200g of water:
______4. .214g of carbon dioxide was dissolved in enough water to make exactly 400ml of solution:
______5. 3.71g of potassium carbonate was dissolved in 325g of water:
______6. 7.83g of ammonium nitrate was dissolved in enough water to make 500ml of solution: MOLARITY PROBLEMS
1. Calculate the mass of solute needed to produce each of the following solutions:
A. 300ml of .100M lithium sulfate B. 125ml of .225M lead(II) acetate
C. 100ml of .400M iron(II) iodide D. 500ml of .033M calcium cyanide
2. What volume of each of the following solutions would be needed to deliver the stated amount of solute?
A. solution is .217M tin(II) sulfate B. solution is .400M NaOH .0341 mol tin(II) sulfate needed .122 mol NaOH needed
C. solution is .125M iron(III) acetate D. solution is .120M CaCl2 .0025 mol iron(III) acetate needed .00333 mol CaCl2 needed
3. 4.233g of chromium(III) nitrate was dissolved in enough water to make 500ml of solution. Determine the molarity of this solution: 4. Explain HOW you would produce 250ml of .100M nickel(II) acetate from the solid compound: COLLIGATIVE PROPERTIES OF SOLUTIONS
We will deal with this topic on a very limited basis… DETERMINATION OF THE MOLARITY OF HCL
PROCEDURE:
1. Obtain and mass a 150 - 250 ml beaker. 2. Add a small quantity of marble chips (5-6 large chips, more if smaller) 3. Mass the beaker and marble chips. 4. Measure the assigned volume of acid in a graduated cylinder. 5. Heat to near boiling, but DO NOT BOIL. 6. Continue heating until the reaction is complete. 7. Decant and dispose of the liquid. 8. Rinse the marble 3 times with water, decanting the liquid. 9. Dry the marble by heating on the hot plate. 10. Allow to cool. 11. Mass the beaker and dry marble. 12. Clean up as instructed.
______Volume of HCl solution.
______Mass of empty beaker.
______ORIGINAL mass of beaker and marble.
______FINAL mass of beaker and marble.
POSTLAB:
1. Write the balanced equation:
2. Calculate the moles of calcium carbonate that reacted:
3. Calculate the moles of HCl that reacted (were in the solution):
4. Calculate the molarity of the HCl solution:
Molarity of HCl = moles HCl L of HCl solution MOLARITY AND REACTIONS
1. Calculate the molarity of 3.22g sodium sulfate dissolved in enough water to make 150ml of solution.
2. Explain how to produce 250ml of .300M KOH.
3. What mass of Fe could be reacted with 200ml of 1.5M HCl?
4. 1.2g NaOH would be neutralized by what volume of .200M sulfuric acid?
5. 4.7g of barium hydroxide was dissolved in enough water to make 200 ml of solution. Determine the molarity of this solution, and the volume that would be needed to react with 15.23ml of .433 M HNO3.
6. Calculate the molarity of NaOH if 34.55 ml was neutralized by 22.77 ml of .1123 M sulfuric acid. 7. What volume of 1.0 M acetic acid (vinegar) would be needed to neutralize a spill that contained 5.00 g NaOH?
8. If 23.45ml of .2095 M KOH is needed to neutralize 31.07 ml of sulfuric acid, what is the concentration of the acid?
9. Calculate the molarity of a barium hydroxide solution, if 45.15 ml is neutralized by 37.25 ml of .442 M hydrochloric acid.
10. What volume of 1.20 M HBr would be needed to react with 48.23 g magnesium carbonate? Solubility of Calcium Hydroxide
Purpose: The purpose of this lab is to determine the solubility of calcium hydroxide.
Procedure: 1. Prepare a burette with the acid solution. 2. Obtain a clean flask. 3. Without mixing, obtain approximately 10 ml of saturated calcium hydroxide solution. Accurately determine the volume and record. 4. Place this solution in a flask. 5. To the flask, add a few drops of indicator, and a small quantity of water. 6. Record the initial volume of the acid solution. 7. Titrate carefully, and record the final volume. 8. Rinse the flask thoroughly. 9. Repeat this procedure for a total of four titrations. (as time allows)
Titration 1 2 3 4 number Volume of saturated Ca(OH)2 solution HCl Molarity
Initial HCl volume
Final HCl volume
HCl volume used
Ca(OH)2 Molarity
Follow-up: 1. Write the balanced equation for the reaction. 2. Complete the table above. On a separate page, in lab report format, show all calculations for ONE titration. 3. Compute an average value for the molarity of saturated Ca(OH)2. 4. If 12.34 ml of .0433 M HCl neutralizes 24.22 ml of a magnesium hydroxide solution, determine the molarity of the magnesium hydroxide solution.
3 BONUS: Given that the density of saturated Ca(OH)2 is 1.02 g/cm , determine the solubility of Ca(OH)2 in the usual units of g/100g water. Solubility of Calcium Hydroxide – FOLLOW UP
As an opportunity to earn up to 5 additional points, complete the following for the data given.
Titration 1 2 3 4 number Volume of saturated 9.92 9.05 10.00 9.51 Ca(OH)2 solution HCl Molarity .0225 .0225 .0225 .0225
Initial HCl volume 45.22 27.87 25.01 33.19
Final HCl volume 25.76 9.73 4.98 14.11
HCl volume used
Ca(OH)2 Molarity
Follow-up:
1. Write the balanced equation for the reaction.
2. Complete the table above. On a separate page, in lab report format, show all calculations for THE FIRST titration (column number one).
3. Compute an average value for the molarity of saturated Ca(OH)2.
4. If 12.34 ml of .0433 M HCl neutralizes 24.22 ml of a magnesium hydroxide solution, determine the molarity of the magnesium hydroxide solution. CHEMISTRY PRE-TEST
A. Review chapters 12 and 13, and all prior materials.
B. Complete the following problems.
1. A chemist wants to make 2.44m KCl. To make this solution, what mass of KCl should be dissolved in 800.0g water?
2. Compute the freezing point of a solution of 20.28g MgF2 in 98.32g water.
3. 25.2g of the nonelectrolyte X was dissolved in 85.34g water. The solution boiled at 101.09oC. Determine the molecular mass of X.
4. What mass of C6H12O6 is present in 150ml of 1.055M C6H12O6?
5. 81.55ml of a lithium hydroxide solution was exactly neutralized by 42.35ml of .0964 M phosphoric acid. Calculate the molarity of the lithium hydroxide solution. Include the balanced equation.
6. What mass of iron(III) hydroxide would be needed to neutralize 49.11 ml of 1.044 M nitric acid? Include the balanced equation.
CHEMISTRY PRE-TEST
A. Review chapters 12 and 13, and all prior materials.
B. Complete the following problems.
1. A chemist wants to make 2.44m KCl. To make this solution, what mass of KCl should be dissolved in 800.0g water?
2. Compute the freezing point of a solution of 20.28g MgF2 in 98.32g water.
3. 25.2g of the nonelectrolyte X was dissolved in 85.34g water. The solution boiled at 101.09oC. Determine the molecular mass of X.
4. What mass of C6H12O6 is present in 150ml of 1.055M C6H12O6?
5. 81.55ml of a lithium hydroxide solution was exactly neutralized by 42.35ml of .0964 M phosphoric acid. Calculate the molarity of the lithium hydroxide solution. Include the balanced equation.
6. What mass of iron(III) hydroxide would be needed to neutralize 49.11 ml of 1.044 M nitric acid? Include the balanced equation.