19. Solution of silver ions react with chloride ion. AgNOsaa)+ NaClag) AgCls NaN

Question

19. Solution of silver ions react with chloride ion. AgNOsaa)+ NaClag) AgCls NaNOs 13 pts. a) A 50.0 ml sample of 0.124 M AgNOs is mixed with 80.0 mL of 0.196 M NaCI. i) What is the limiting reactant? Limiting reagent- ii) How many grams of solid AgCl are prepared? Grams of AgCI- b) In the lab we titrated an acetic acid solution with NaOH. HC2H302(ag)+ NaOH(ag)NaC2H302(a)+H2O i) If a 10.0 mL sample of HC H3O2 (M 60.05 g) required 24.2 ml of 0.7850 M NaOH then: What is the molarity of the HC2Ha02 solution? Molarity- ii) If the density of a HC2H,02 solution is 1.08 g / mL, and it is 16.6% HC2H02, what is its molarity? Molarity 20. How many liters of gas are generated by each of the following reactions? 8 pts. a) A 44.5 g sample of HgO is heated and the gas is collected at 800 mm of Hg and 365°C. Liters of 02 collected- b) A 76.0 g sample 15.0% hydrogen peroxide (H2O2 by mass, density-1.02 g/mL) was treated with FeCla (catalyst) to give O- If the gas is collected at STP, how many liters of O; could theoretically be collected? Liters of O2 collected at STP

Explanation / Answer

Part a

Moles of AgNO3 = molarity x volume

= 0.124 mol/L x 0.050 L

= 0.0062 mol

Moles of NaCl = 0.196 mol/L x 0.080 L

= 0.01568 mol

From the stoichiometry of the reaction

1 mol of AgNO3 reacts with = 1 mol of NaCl

Moles of AgNO3 < moles of NaCl

Limiting reactant = AgNO3

Moles of AgCl formed = moles of AgNO3 consumed

= 0.0062 mol

Mass of AgCl formed = 0.0062 mol x 143.32 g/mol

= 0.888 g

Part b

Moles of NaOH = 0.0242 L x 0.7850 mol/L

= 0.018997 mol

moles of HC2H3O2 = 0.018997 mol

Total volume = 10 + 24.2 = 34.2 = 0.0342 L

Molarity = moles of HC2H3O2 / Total volume

= 0.018997/0.0342

= 0.555 M

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