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(b) How many moles of KMnO4 are present in 250 mL of a 0.0475 M solution?

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(a) Calculate the molarity of a solution made by dissolving 0.750 grams of Na 2SO4 in enough water to form exactly 850 mL of solution.

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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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Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions?

(e) H2(g) + CuCl2(aq) →

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Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions? 

(d) Pt(s) + HBr(aq) →

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Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions? 

(c) Cr(s) + NiSO4(aq) →

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Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions?

(b) Cu(s) + Cr(CH3COO)3(aq) →

 

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Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions?
(a) Mn(s) + NiCl2(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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Write balanced molecular and net ionic equations for the reactions of (b) chromium with hydrobromic acid

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