CHEM151Take-home Q10 Key

Chemistry (MasteringChemistry Series)

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Name Take‐Home Quiz #10 (DUE Monday November 17th, 2008) Key Date Score Show ALL work to get full credit: 1) (1 point) How many grams of sodium nitrate, NaNO3, are needed to make 250.0 ml of 1.2 M solution? 250.0 1 1000 1.2 1 85.01 1 25.5 2) (1 point) How many milliliters of 13 M nitric acid, HNO3 (aq) is needed to make 500.0 ml of 0.993 M solution? 13 13 0.993 · 500.0 13 3) (1 points) How many grams of precipitate is produced when 10.0 ml of 1.32 M silver nitrate, AgNO3 (aq), reacts with an excess of MgCl2 (aq)? 2 2 10.0 1 1000 1.32 1 2 2 143.3182 1 1.89 4) (3 points) How many grams of silver metal would precipitate if 1.00 g of Zinc metal was added to 25.0 ml of 1.46 M silver nitrate, AgNO3(aq)? 2 : 1.00 : 25.0 1 1000 1 65.39 1.46 1 2 2 1 107.8682 1 2 2 . 107.8682 1 3.94 a. Identify the limiting reactant. Zn is the limiting reactant. It produces the least amount of product. b. What is the percent yield if 2.96 g of silver metal was actually produced? 2.96 100 100 .% 3.30 5) (1 point) What is the molarity of a sodium hydroxide solution, NaOH(aq), if it took 14.50 ml to titrate 10.00 ml of 0.9967 M acetic acid, CH3COOH(aq)? 10.00 1 1000 0.9967 1 0.009967 0.01450 1 . 1 0.009967 6) (1 point) What volume of 1.32 M potassium hydroxide, KOH (aq), is needed to completely react with 15.3 ml of 1.043 M MgSO4 (aq)? 2 15.3 1 1000 . 1.043 1 . 1 2 1.32 1 7) (2 points) What is the empirical formula of ibuprofen given the following: carbon has 75.7 mass%, hydrogen has 8.8 mass%, and oxygen has 15.5 mass%. Assume 100 g sample: 75.7 . 6.303 0.9688 6.5 (This one can be a bit tricky. It comes out to 6.50 so leave it as 6.5. It will make more sense when you get to the molecular formula portion. Usually when doing these types of problems you will get whole numbers or halves, i,e, X.5. If you have a X.5 leave it as is. You will likely need to double when you get the molecular formula) 8.8 15.5 . 8.713 0.9688 0.9688 0.9688 9 1 . a. Given the molecular weight of ibuprofen is 206.31 g/mol, what is the molecular formula? The molar mass of the empirical formula from above: 6.5 206.31 Therefore the Molecular Formula is: 103.155 . 9 . 103.155 2 ...
View Full Document

This document was uploaded on 09/27/2011.

Ask a homework question - tutors are online