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 0.669 g. a 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) b) 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.) c) Calculate the percentage of sodium chloride in the original unknown mixture. %MaCl

Explanation / Answer

NaCl + NaNO3 + AgNO3 -----> AgCl + 2 NaNo3
in the solution we observe Na+ , NO3- and AgCl solid
net ionic equation is
Ag+ (aq) + Cl-(aq) -----> AgCl(s)
mass of AgCl = 0.669 g
number of moles of AgCl = 0.669/143.32 = 0.004668 moles
so number of moles of NaCl = 0.004668
because 1 mole of NaCl produces 1 mole of AgCl
mass of NaCl = 0.004668 * 58.5 = 0.2731 g
percentage of NaCl = 0.2731/1.5 *100 = 18.21 %

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