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Assign oxidation states for all atoms in each of the following compounds.

f. Mg2P2O7

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Assign oxidation states for all atoms in each of the following compounds.

e. HAsO2

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Assign oxidation states for all atoms in each of the following compounds.

d. As4

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Assign oxidation states for all atoms in each of the following compounds.

c. NaBiO3

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Assign oxidation states for all atoms in each of the following compounds.

b. As2O3

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Assign oxidation states for all atoms in each of the following compounds.

a. UO22+

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The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.

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A student titrates an unknown amount of potassium hydrogen phthalate (KHC 8H4O4, often abbreviated KHP) with 20.46 mL of a 0.1000 M NaOH solution. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?

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A 30.0-mL sample of an unknown strong base is neutralized after the addition of 12.0 mL of a 0.150 M HNO3 solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.

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What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?

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A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point.

b. If the density of the vinegar is 1.006 g/cm 3, what is the mass percent of acetic acid in the vinegar?

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A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point.

a. What is the molarity of the acetic acid?

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A 25.00-mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?

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A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Is the resulting solution neutral? If not, calculate the concentration of excess H+ or OH ions left in solution.

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Hydrochloric acid (75.0 mL of 0.250 M) is added to 225.0 mL of 0.0550 M Ba(OH)  2 solution. What is the concentration of the excess H+ or OH ions left in this solution?

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What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?

c. 0.250 M KOH

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What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?

b. 0.0500 M Sr(OH)2

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What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?

a. 0.100 M NaOH

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What acid and what strong base would react in aqueous solution to produce the following salts in the formula equation? Write the balanced formula equation for each reaction.

c. calcium iodide

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What acid and what strong base would react in aqueous solution to produce the following salts in the formula equation? Write the balanced formula equation for each reaction.

b. cesium nitrate

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What acid and what strong base would react in aqueous solution to produce the following salts in the formula equation? Write the balanced formula equation for each reaction.

a. potassium perchlorate

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Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions.

c. Ca(OH)2(aq) + HCl(aq) →

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Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions.

b. HC2H3O2(aq) + KOH(aq) →

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Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions.

a. HNO3(aq) + Al(OH3)(s) →

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You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.

c. Calculate the percent sodium chloride in the original unknown mixture.

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