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11 Dec 2019

It is desired to neutralize a solution X that contains a mixture of potassium chromate and sulfuric acid. Titration of 14.9 mL X with 0.127 M barium nitrate required 49.9 mL of the latter. The resulting precipitate, containing a mixture of BaCrO₄ and BaSO₄, was dried and found to weigh 1.520 g. How much 0.118 M sodium hydroxide should be used to neutralize 14.9 mL solution X?

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13 Dec 2019

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It is desired to neutralize a solution X that contains a mixture of potassium chloride and hydrobromic acid. Titration of 13.6 mL X with 0.107 M silver nitrate required 56.6 mL of the latter. The resulting precipitate, containing a mixture of AgCl and AgBr, was dried and found to weigh 1.090 g. How much 0.131 M sodium hydroxide should be used to neutralize 13.6 mL solution X?

Hello Chegg family i have a few titration and oxidation problems. Thank You!

1.) What volume of a 0.367 M hydrochloric acid solution is required to neutralize 14.3 mL of a 0.177 Msodium hydroxide solution?
??mL hydrochloric acid

What volume of a 0.142 M barium hydroxide solution is required to neutralize 24.1 mL of a 0.154 Mperchloric acid solution?
??mL barium hydroxide

2.) An aqueous solution of hydrochloric acid is standardized by titration with a 0.177 M solution of calcium hydroxide.
If 14.3 mL of base are required to neutralize 27.8 mL of the acid, what is the molarity of the hydrochloric acid solution?
??M hydrochloric acid

An aqueous solution of barium hydroxide is standardized by titration with a 0.142 M solution of perchloric acid.
If 24.1 mL of base are required to neutralize 13.6 mL of the acid, what is the molarity of the barium hydroxide solution?
??M barium hydroxide

3.) Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as aprimary standard. It has the unwieldy formula of KHC₈H₄O₄. This is often written in shorthand notation as KHP.
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A solution containing a mixture of 0.0444 M potassium chromate (K2CrO4) and 0.0664 M sodium oxalate (Na2C2O4) was titrated with a solution of barium chloride (BaCl2) for the purpose of separating CrO42â and C2O42â by precipitation with the Ba2 cation. Answer the following questions regarding this system. The solubility product constants (Ksp) for BaCrO4 and BaC2O4 are 2.10 Ã 10-10 and 1.30 Ã 10-6, respectively.

A.) Which barium salt will precipitate first?

B.) What concentration of Ba2+ must be present for BaCrO4 to begin precipiating?

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