This question has multiple parts. Work all the parts to get the most points. You

Question

This question has multiple parts. Work all the parts to get the most points. You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.724 g. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). (Enter multiple answers as a comma-separated list.) ______________ Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) _______________ + _______________ rightarrow ___________ Calculate the percentage of sodium chloride in the original unknown mixture. _________________ % NaCl

Explanation / Answer

a. Ag+, Cl-, Na+, NO3-

b. 2Na+ + 2NO3- + Cl- + Ag+ ----------------> AgCl(s) + NaNO3(aq.)

c. NaCl ---------->AgCl

58.5g of NaCl corresponds to 143.3 g of AgCl, so 0.724g of AgCl would be produced from

= (58.5x 0.724)/143.3 = 0.295 g

1.50g of mixture contains 0.295 g of NaCl.

So, the percentage of NaCl = (0.295/1.50)x100 = 19.6%

percentage of NaCl = 19.6%

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