Chem._Test_1 Work Sheets

# Chem._Test_1 Work Sheets - 3.15 Concept Worksheet for...

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3.15 Concept Worksheet for Concentration of Mixtures For mixtures, solute is added from both of the solutions. To determine the final concentration, the total number of moles of solute is first determined, then this is divided by the total volume. In equation form, this is M 1 V 1 + M 2 V 2 = M t V t . Practice Problems: 1. What is the final concentration of NaOH in a mixture of 100ml of 0.50M NaOH and 100 ml of 0.30M NaOH? 2. What is the final [HCl] when I mix 200ml of 0.25M HCl and 300ml of 0.55M HCl? 3. I mix 100ml of 2.5M NaOH and 400ml of 1.5M NaOH. What is the [NaOH] in the mixture? 4. I mix 200ml of 2.5M HCl and 500ml of 1.0M HCl. What is the concentration of HCl in the mixture? 5. If I mix 500ml of 0.35M HCl and 500ml of 0.65M HCl, what is the final [HCl]? Answers: 1. 0.40M NaOH 2. 0.43M HCl 3. 1.7 M NaOH 4. 1.4 M HCl 5. 0.45M HCl

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3.14 Concept Worksheet for Dilutions When water is added to a solution, the total volume increases and the concentration of the solute in the original solution decreases. We can determine the final concentration by calculating the number of moles of solute in the original solution and then dividing that by the total volume. In formula form, this is M 1 V 1 = M t V t or, better, M t = M 1 *V 1 /V t . Practice Problems: 1. What is the final concentration when 100 ml of 0.55M HCl is diluted to a total of 500ml. 2. What is the final concentration when 200ml of water are added to 300ml of 0.25M NaOH? 3. What is concentration of the diluted solution made by mixing 200ml of 0.65M HCl and 800 ml of water? 4. What is the concentration of the diluted solution when 150ml of 0.85M HCl is diluted to 750ml? 5. What volume of water do I need to add to 200ml of 0.60M HCl in order to dilute the solution to 0.30M HCl 6. To what total volume do I need to dilute 100ml of 6.0M NaOH in order to have a 1.5M solution? Answers: 1. 0.11M HCl 2. 0.10M NaOH 3. 0.13M HCl 4. 0.17M HCl 5. 200 ml of water 6. 400ml of total solution
3.13 Concept Worksheet for Yield In many reactions, we know the amount of both starting reagents. We can calculate two quantities of product using stoichiometry but the reaction can only produce the smallest of these until one of the reagents is used up. The reagent that is used up first is called the limiting reagent. The amount of product that can be produced from that amount of reagent is called the theoretical or potential yield. The reagent that is left over is called the excess reagent. If the actual yield is measured, then the % yield can be calculated (actual divided by theoretical). Practice Problems: 1. What is the potential yield of Mg(OH) 2 when 100ml of 2.5M NaOH and 15g of MgCl 2 are reacted? 2. What is the limiting reagent and the theoretical yield of water when 2.5g of H 2 and 8.6g of O 2 are reacted? 3.

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## This note was uploaded on 01/16/2009 for the course CHEM 1411 taught by Professor Moses during the Fall '08 term at A.T. Still University.

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Chem._Test_1 Work Sheets - 3.15 Concept Worksheet for...

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