It is desired to neutralize a solution X that contains a mixture of potassium chromate and hydrochloric acid. Titration of 11.3 mL X with 0.104 M silver nitraterequired 78.6 mL of the latter. The resulting precipitate, containing a mixture of Ag2CrO4 and AgCl, was dried and found to weigh 1.250 g. How much 0.107 M sodium hydroxide should be used to neutralize 11.3 mL solution X?

Question 22 of 30 Submit A 185.0 mL sample of 1.200 M Pb(NO3)2 is mixed with 123.50 mL of 1.500 M NaCI, and the PbCl, precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr, precipitate is also collected and dried. What is the mass (in grams) of the PbBr, precipitate, assuming the yield in each precipitation step is 100%? 1 4 6. C 7 +/- x 10 0 Tap here or pull up for additional resources LO 00

Solid potassium hydroxide is slowly added to 150 mL of a 0.0538 M iron(II) acetate solution. The concentration of hydroxide ion required to just initiate precipitation is  M.

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A 20.0-mLmL sample of 0.150 MKOH is titrated with 0.125 MHClO4 solution. Calculate the pHpH after the following volumes of acid have been added. 23.5 mL Express your answer using two decimal places.   31.0 mL Express your answer using two decimal places.

How many grams of NaCl to precipitate Ag+ from 2.50 x 102 mL of .0113M AgNO3?

Solid ammonium chloride is slowly added to 125 mL of a lead(II) acetate solution until the concentration of chloride ion is 0.0284 M. The maximum amount of lead ion remaining in solution is  M.

The formula H₂SO4 + 2 KOH --> K₂SO4 + 2 H₂O describes the reaction between sulfuric acid and potassium hydroxide. In the titration done, 20 mL of KOH with an unknown concentration is put into a flask with bromthymol blue indicator. The KOH solution was titrated with a 0.25 M H₂SO4 solution. Three trials were performed and each trial yielded to an endpoint of yellow-colored solution, which is the desired endpoint. After three trials, the following readings were obtained: 15.5, 15.1, and 14.9 mL respectively. Calculate the molarity of Potassium hydroxide. (Answer must be rounded off to 2 decimal places)

A 0.6407g sample containing chloride and iodide ions gave a silver halide precipitate weighing 0.4430g. This precipitate was then strongly heated in a stream of chlorine gas to convert the AgI to AgCl; on completion of this treatment, the precipitate weighed 0.3181g. Calculate the percentage of chloride and iodide in the sample.

An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution?   2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution?   3. What is the concentration of Ag+ in solution?