1. Two chemists are using water in sepratory funnels to wash out salts from each of their crude reaction mixtures. A wash with 100. mL of water removes approximately 85% of the salts. Chemist 1 does one wash with 300. mL, while chemist 2 does three separate washes of 100. mL each. While each chemist used a total of 300. mL of water, one of them removed more salts. Suppose that each crude reaction mixture had 10.0 g of salt initially, calculate the amount of salt remaining for both chemists? Show your work. Which chemist removed more salt?

1. Two chemists are using water in sepratory funnels to wash out salts from each of their crude reaction mixtures. A wash with 100. mL of water removes approximately 85% of the salts. Chemist 1 does one wash with 300. mL, while chemist 2 does three separate washes of 100. mL each. While each chemist used a total of 300. mL of water, one of them removed more salts. Suppose that each crude reaction mixture had 10.0 g of salt initially, calculate the amount of salt remaining for both chemists? Show your work. Which chemist removed more salt?

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter2: Matter

Section: Chapter Questions

Problem 21A

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The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry textbook estimates that if 1.00 × 108 tons Mg were taken out of the sea each year, it would take one million years for the Mg concentration to drop to 0.12%. Do sufficient calculations to either verify or refute this statement. Assume that Earth is a sphere with a diameter of 8000 mi, 67% of which is covered by oceans to a depth of 1 mi, and that no Mg is washed back into the oceans at any time.
pour it 2. Still sleepy from a late night studying, you take the milk out of the refrigerator and pour it on your lemon juice to milk to make paneer (fresh cheese). As a group, craft a chemical explanation for the fact of coagulated milk onto your cereal. The last time you saw milk coagulate like that was when you added breakfast cereal. Unfortunately, by the time you notice the funny smell you have already poured clumps lemon juice to milk to make paneer (fresh cheese). As a group, craft a chemical explanation foea added that spoiled milk coagulates.
6. Write the expression for Kc for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. a. CH4 (g) + H2S (g) → CS2(g) + H2 (g) HF + F¯ (aq) b. (aq) ⇒ H* (aq) c. Ti (s) + Cl2 (g) → TiCl4 (1) d. HCI (aq) + O2 (g) → H₂O (1) + 2 Cl2 (g)
3. Solubility data for copper(II) nitrate (Cu(NO3)2) and potassium nitrate (KNO3) at different temperatures is shown below. The values are for grams of compound per 10 milliliters of water. 0°C 20°C 40°C 60°C 80°C 100°C Cu(NO3)2 8.35 12.5 16.3 18.2 20.8 24.7 KNO3 1.3 3.2 6.4 11.0 16.9 24.6 Remember that the solubility of a compound refers the maximum amount of compound that can be dissolved in a particular solvent at a particular temperature. So for example, the maximum amount of copper(II) nitrate that can be dissolved in 10 mL of water at 80°C is 20.8 grams, and the maximum amount of potassium nitrate that can be dissolved in 10 mL of water at 80°C is 16.9 grams. a. How much potassium nitrate could you dissolve in 25 milliliters of water at 60°C based on the data in the table above? (Hint: use the solubility as a conversion factor in the calculation.) b. Could you dissolve 3.0 grams of potassium nitrate in 5 milliliters of water at 60°C? Indicate Yes or No. Explain your answer below.
4. At 20°C, acetaminophen has a solubility of about 1.5 g/100 mL in water. If you recrystallize 5.00g of crude acetaminophen in 50 mL of water. What is the maximum mass of solid acetaminophen you would expect to recover after cooling to 20°C? 4.25 g 3.5 g 5.75 g 6.5 g
Calculate the each initial CONCENTRATION for Pb(NO3)2 and KI before filling-out this chart. (Refer t Steps 1 and 2 of the procedure. Use the formula for Molarity to calculate the concentration of each salt after preparing the solution from the solid crystals dissolved in 100 mL of water. Do this for Lead (II) Nitrate and KI separately. Then use the dilution formula (starting with the initial concentration) for EACH beaker – each will have a the same total volume, but different volume of each solution added for each beaker. In short, FOR EACH BEAKER, multiple the concentration for Pb(NO3)2 with the concentration of KI.
3. A student forgot to pre-measure the mass of the second evaporating dish prior to decanting the salt water mixture into it. Can the student weigh another evaporating dish of the same size and use its mass instead? 4 By what means could you separate a mixture of benzoic acid and sodium nitrate? 65 4x 12:05 AM 6/30/2022
2. Pyrite (FeS2) can be leached by oxygen in sulfuric acid solution to form ferric sulfate. Write the balanced chemical reaction in ionic and neutral forms and include the phases of the reactants and products.
1. A candle is placed on one pan of a balance, and an equal weight is placed on the other pan. What would happen if you lit up the candle and waited for a while? Suppose the candle was placed in a large, sealed jar that allowed it to burn for several minutes before running out of oxygen. The candle and jar are balanced by an equal weight. In this situation, what would happen if you lit up the candle and waited?
A student follows a lab protocol that asks them to make an ‘alcohol’ solution for an experiment. They make a 1.00 L solution by adding 575 g of an alcohol to water. Later they realize that there were three different alcohols sitting on the lab bench and they’re not sure which one they used. The alcohols are: methanol (CH3OH), ethanol (C2H5OH), and butanol (C4H9OH). They decide to boil the solution and they find that it boils at 106.40 °C. Using this information determine which alcohol the student used to make their solution. Density of water is 1.00 g/mL, Kb = 0.513 K/mc. Hint: you need to consider the molar masses of your alcohols.
1)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain?Express your answer to the correct number of significant figures. 2)Suppose the Na2CO3 solution described in Question 1 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?
A sample of pure acetyl salicylic acid had a mass of 0.268 grams. It was dissolved in NaOH and diluted to 500.00 mL in a volumetric flask. a. What is the concentration of aspirin in the solution? If an 8.00 mL sample of this solution was pipetted into a volumetric flask and diluted to 100.00 mL, what is the concentrated of aspirin after this dilution? b.

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