Solve Chemistry HW: Silver Ions + H2SO4 | Help with Answers

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Discussion Overview

The discussion revolves around two chemistry homework questions involving stoichiometry and titration calculations. The first question pertains to the precipitation of silver ions using sodium chloride, while the second question involves determining the concentration of sulfuric acid after titration with sodium hydroxide.

Discussion Character

  • Homework-related
  • Mathematical reasoning

Main Points Raised

  • One participant outlines the first question regarding the precipitation of silver ions and asks how many grams of NaCl are needed to precipitate silver from a given volume and concentration of AgNO3 solution.
  • Another participant suggests that the problem involves stoichiometry, indicating the need to calculate moles of silver and chloride ions and subsequently determine the mass of NaCl required.
  • The second question involves titration, where a participant notes the volume of NaOH used and the need to find the concentration of H2SO4, referencing the balanced chemical equation for the neutralization reaction.
  • A link to a resource on titration calculations is provided by one participant as a potential aid for solving the second question.
  • One participant points out that the original poster has previously asked similar questions and received hints, implying a need for further clarification or guidance.

Areas of Agreement / Disagreement

Participants generally agree on the nature of the problems as stoichiometric calculations, but there is no consensus on the specific methods or solutions to the questions posed.

Contextual Notes

Some assumptions regarding the completeness of reactions and the precision of measurements may not be explicitly stated. The discussion does not resolve the mathematical steps necessary for the calculations.

kevin0788
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Hi, i have 2 questions about my chemistry homework i can not figure out
The first question is:

1)Silver ions can be precipitated from an aqueous solutions by the addition of aqueous chloride:

Ag+(aq) + Cl-(aq) ---->AgCl(s)

Silver chloride is virtualy insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0mL of 0.326 M AgNo3 solution to completely precititate the silver?

The second question is:

2) A 31.5 mL aliquot of H2SO4(aq) of unknown concentration was titrated with 0.0134 M NaOH(aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was_____. (be sure to write a balanced chemical equation for the neutralization reaction.)

I already balanced the equation.

H2SO4 + 2NaOH ------> Na2SO4 + 2H2O


Can anybody tell me how to go about solving either of these questions?
 
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Basically both questions are simple stoichiometry with moles/mass and volume/moles conversions.

kevin0788 said:
Ag+(aq) + Cl-(aq) ---->AgCl(s)

Silver chloride is virtualy insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0mL of 0.326 M AgNo3 solution to completely precititate the silver?

How many moles of silver? How many moles of chloride needed? What mass?

2) A 31.5 mL aliquot of H2SO4(aq) of unknown concentration was titrated with 0.0134 M NaOH(aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was_____. (be sure to write a balanced chemical equation for the neutralization reaction.)

http://www.titrations.info/titration-calculation

--
methods
 
Chemistry

Hi, i have 2 questions about my chemistry homework i can not figure out
The first question is:

1)Silver ions can be precipitated from an aqueous solutions by the addition of aqueous chloride:

Ag+(aq) + Cl-(aq) ---->AgCl(s)

Silver chloride is virtualy insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0mL of 0.326 M AgNo3 solution to completely precititate the silver?

The second question is:

2) A 31.5 mL aliquot of H2SO4(aq) of unknown concentration was titrated with 0.0134 M NaOH(aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was_____. (be sure to write a balanced chemical equation for the neutralization reaction.)

I already balanced the equation.

H2SO4 + 2NaOH ------> Na2SO4 + 2H2O


Can anybody tell me how to go about solving either of these questions?
 

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