Precipitation Stoichiometry PL 1. When solutions of lead(II) nitrate and aluminum chloride are mixed, a precipitate forms. Write a balanced formula equation for the reaction. a. (aq) +3 3 Pb² (NO3) (2) 2A1+ ³ (1.1) 2A1 (NO 3 ) 2 + 3 PbCl 2 (5) b. What volume of a 0.200 M lead(II) nitrate solution is needed to completely form a precipitate when added to 2.48 mL of 0.300 M aluminum chloride? C. 2.48mL .002484 0.200 What is the mass of precipitate formed in (b)? 2. What mass of precipitate is formed when 71.3 mL of 0.500 M iron(III) nitrate are mixed with 112 mL of 0.800 M sodium carbonate? 3. What volume of 2.0 M K₂SO, is needed to react with an excess of Zn(CH3CO2)2 to produce 25.0 grams of zinc sulfate? - 4. What mass of sodium chromate is required to precipitate all of the silver ions from 75.0 mL of a 0.100 M silver nitrate solution? 5. What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M aluminum nitrate is added to 200.0 mL of 0.100 M KOH? n 4.5: Acid Chemical

Precipitation Stoichiometry PL 1. When solutions of lead(II) nitrate and aluminum chloride are mixed, a precipitate forms. Write a balanced formula equation for the reaction. a. (aq) +3 3 Pb² (NO3) (2) 2A1+ ³ (1.1) 2A1 (NO 3 ) 2 + 3 PbCl 2 (5) b. What volume of a 0.200 M lead(II) nitrate solution is needed to completely form a precipitate when added to 2.48 mL of 0.300 M aluminum chloride? C. 2.48mL .002484 0.200 What is the mass of precipitate formed in (b)? 2. What mass of precipitate is formed when 71.3 mL of 0.500 M iron(III) nitrate are mixed with 112 mL of 0.800 M sodium carbonate? 3. What volume of 2.0 M K₂SO, is needed to react with an excess of Zn(CH3CO2)2 to produce 25.0 grams of zinc sulfate? - 4. What mass of sodium chromate is required to precipitate all of the silver ions from 75.0 mL of a 0.100 M silver nitrate solution? 5. What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M aluminum nitrate is added to 200.0 mL of 0.100 M KOH? n 4.5: Acid Chemical

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 119AE: Chlorisondamine chloride (C14H20Cl6N2) is a drug used in the treatment of hypertension. A 1.28-g...

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Sodium bicarbonate and acetic acid react according to the equation NaHCO3(aq) + CH3CO2H(aq) NaCH3CO2(aq) + CO2(g) + H2O(l) What mass of sodium acetate can be obtained from mixing 15.0 g of NaHCO3 with 125 mL of 0.15 M acetic acid?
Lactic acid, C3H6O3 is the acid present in sour milk. A 0.100-g sample of pure lactic acid requires 12.95 mL of 0.0857 M sodium hydroxide for complete reaction. How many moles of hydroxide ion are required to neutralize one mole of lactic acid?
Potassium permanganate (KMnO4) solutions are used for the determination of Fe2+ in samples of unknown concentration. As a laboratory assistant, you are supposed to prepare 500 mL of a 0.1000 M KMnO4 solution. What mass of KMnO4, in grams, do you need?
Arsenic acid, H3AsO4, is a poisonous acid that has been used in the treatment of wood to prevent insect damage. Arsenic acid has three acidic protons. Say you take a 25.00-mL sample of arsenic acid and prepare it for titration with NaOH by adding 25.00 mL of water. The complete neutralization of this solution requires the addition of 53.07 mL of 0.6441 M NaOH solution. Write the balanced chemical reaction for the titration, and calculate the molarity of the arsenic acid sample.
You can dissolve an aluminum soft drink can in an aqueous base such as potassium hydroxide. 2 Al(s) + 2 KOH(aq) + 6 H2O(l) 2 KAI(OH)4(aq) + 3 H2(g) If you place 2.05 g of aluminum in a beaker with 185 mL of 1.35 M KOH, will any aluminum remain? What mass of KAI(OH)4 is produced?
Potassium hydrogen phthalate, KHCgH4O4, is used to standardize solutions of bases. The acidic anion reacts with strong bases according to the following net ionic equation: HCgH4O4(aq) + OH(aq) CgH4O42(aq) + H2O(l) If a 0.902-g sample of potassium hydrogen phthalate is dissolved in water and titrated to the equivalence point with 26.45 mL of NaOH(aq), what is the molar concentration of the NaOH?
Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride, CaCL2. To precipitate the calcium ion from the resulting solution, an excess of potassium oxalate was added. The precipitate of calcium oxalate, CaC2O4, weighed 1.437 g. What was the molarity of CaCl2 in the solution?
Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?
What is an acid-base reaction? Strong bases are soluble ionic compounds that contain the hydroxide ion. List the strong bases. When a strong base reacts with an acid, what is always produced? Explain the terms titration, stoichiometric point, neutralization, and standardization.
A noncarbonated soft drink contains an unknown amount of citric acid, H3C6H5O7. lf 100. mL of the soft drink requires 33.51 mL of 0.0102 M NaOH to neutralize the citric add completely, what mass of citric acid does the soft drink contain per 100. mL? The reaction of citric acid and NaOH is H3C6H5O7(aq) + 3 NaOH(aq) Na3C6H5O7(aq) + 3 H2O()
A 0.608-g sample of fertilizer contained nitrogen as ammonium sulfate, (NH4)2SO4. It was analyzed for nitrogen by heating with sodium hydroxide. (NH4)2SO4(s)+2NaOH(aq)Na2SO4(aq)+2H2O(l)+2NH3(g) The ammonia was collected in 46.3 mL of 0.213 M HCl (hydrochloric acid), with which it reacted. NH3(g)+HCl(aq)NH4Cl(aq) This solution was titrated for excess hydrochloric acid with 44.3 mL of 0.128 M NaOH. NaOH(aq)+HCl(aq)NaCl(aq)+H2O(l) What is the percentage of nitrogen in the fertilizer?
Potassium hydrogen phthalate (abbreviated as KHP) has the molecular formula KHC8H4O4 and a molar mass of 204.22 g/mol. KHP has one acidic hydrogen. A solid sample of KHP is dissolved in 50 mL of water and titrated to the equivalence point with 22.90 mL of a 0.5010 M NaOH solution. How many grams of KHP were used in the titration?

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