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18 Dec 2019

A student dissolved 0.13 g of a sample containing an unkinown amount of cholride ion in 50 mL of water. She then added 6 drops of Na2CrO4 and titrated the solution using a 0.049 M solution of silver nitrate. She obtained the following data. Initial buret reading = 0.02 mLFinal buret reading = 21.46 mLa. What volune of tirant (silver nitrate, AgNo3) was used?b. How many moles of silver were added to the solution?c. How many moles of chloride were present in the unknown?d. What mass of cholride was present in the unknown?e. What was the mass percentage of cholride present int he original sample?Please show work.

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Related questions

So pretty much I have a balanced equation ofNaCl(aq)+AgNO3(aq)---NaNO3(aq)+AgCl(s). There is a mystery solutionthat has an unknown amout of AgNO3 and the problem wants me to findthe mass of AgNO3 present in the mystery solution. So if I have98.623 mL, 204.874g of mystery solution, 56.685 mL, 251.892g ofNaCl, and 54.646 mL, 365.003g AgNO3. The molar mass of AgCl is143.323, molar mass of AgNO3 is 169.874. This is a limitingreactant problem. The only hint I get is how can you determine themass of silver nitrate dissolved in a solution of unknownconcentration based on the chemistry of the reaction between silvernitrate and sodium chloride to produce solid silver chloride andaqueous sodium nitrate? The answer should be around 2.xx(hundreths) something. Also if you were to perform this in lab whatsoltuion would you pour into what and about what process would yougo through to find mystery soltuion?What is the mass ofAgNO3 that is present in mystery solution?

Sorry for Image size, I need help onthe last three problems, it is something that my girlfriend and Iare struggling on.

Analysis of an Unknown Chloride

1. A student performed this experiment and obtained the following concentration values: 0.02813 M, 0.02802 M, and 0.02788 M.

a. What is the mean concentration? ____________ M

b. What is the standard deviation of these results? ____________ M

2. A 10.00 mL diluted chloride sample required 13.89 mL of 0.02014 M AgNO3 to reach the Fajans endpoint.

a. How many moles of Cl− ion were present in the sample? (Use Eqs. 2 and 3.) ____________ moles Cl−

b. What was the concentration of chloride in the diluted solution? ____________ M

3. How would the following errors affect the concentration of Cl− obtained in Question 2b? Give your reasoning in each case.

a. The student read the molarity of AgNO3 as 0.02104 M instead of 0.02014 M.

b. The student was past the endpoint of the titration when he took the final buret reading.

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