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Indicate the concentration of each ion present in the solution formed by mixing (c) 3.60 g KCl in 75.0 mL of 0.250 M CaCl2 solution. Assume that the volumes are additive.

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Indicate the concentration of each ion present in the solution formed by mixing (b) 44.0 mL of 0.100 M and Na2SO4 and 25.0 mL of 0.150 M KCl. Assume that the volumes are additive.

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Indicate the concentration of each ion or molecule present in the following solutions: (d) a mixture of 45.0 mL of 0.272 M NaCl and 65.0 mL of 0.0247 M (NH4)2CO3. Assume that the volumes are additive.

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Indicate the concentration of each ion or molecule present in the following solutions: (c) 0.0150 M C6H12O6

Assume that the volumes are additive.

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Indicate the concentration of each ion or molecule present in the following solutions: (b) 1.3 x 10–2 MgSO4

Assume that the volumes are additive.

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Indicate the concentration of each ion or molecule present in the following solutions: (a) 0.25 M NaNO3

Assume that the volumes are additive.

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A person suffering from hyponatremia has a sodium ion concentration in the blood of 0.118 M and a total blood volume of 4.6 L. What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to 0.138 M, assuming no change in blood volume?

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The average adult human male has a total blood volume of 5.0 L. If the concentration of sodium ion in this average individual is 0.135 M, what is the mass of sodium ion circulating in the blood?

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(c) A certain volume of a 0.50 M solution contains 4.5 g of a salt. What mass of the salt is present in the same volume of a 2.50 M solution?

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(b) Suppose you prepare 500 mL of a 0.10 M aqueous solution of some salt and let it sit out, uncovered, for a long time, and some water evaporates. What happens to the concentration of the solution left in the container?

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(a) Suppose you prepare 500 mL of a 0.10 M solution of some salt and then spill some of it. What happens to the concentration of the solution left in the container?

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(b) What is the difference between 0.50 mol HCl and 0.50 M HCl?

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(a) Is the concentration of a solution an intensive or an extensive property?

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(a) Use the following reactions to prepare an activity series for the halogens:

Br2 (aq) + 2 NaI (aq) → 2 NaBr (aq) + I 2 (aq)

Cl2 (aq) + 2 NaBr (aq) → 2 NaCl (aq) + Br 2 (aq)

 

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Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (e) aluminum metal is added to a solution  of cobalt(II) sulfate.

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Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride

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Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (c) hydrobromic acid is added to tin metal

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Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (b) zinc metal is added to a solution of magnesium sulfate

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Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (a) Iron metal is added to a solution of copper(II) nitrate

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Write balanced molecular and net ionic equations for the reactions of (d) acetic acid, CH3COOH, with zinc.

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Write balanced molecular and net ionic equations for the reactions of (c) hydrobromic acid with magnesium

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Write balanced molecular and net ionic equations for the reactions of (b) dilute sulfuric acid with iron

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Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel

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Write balanced molecular and net ionic equations for the reactions of (d) aluminum with formic acid, HCOOH.

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Write balanced molecular and net ionic equations for the reactions of (c) tin with hydrochloric acid

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