The mass percent of chloride ion in a 25.00 mL sample of seawater was determined by titrating the sample with silver nitrate, causing precipitation of silver chloride. It requires 42.58 mL of 0.2997 M silver nitrate solution to reach the equivalence point. 25. Write a balanced chemical equation for the reaction that occurs. 26. What is the mass % of chloride ion in the water (density of the solution is 1.025 g/mL)?

A. How many mL of a 0.171 M aqueous solution of nickel(II) nitrate, Ni(NO3)2, must be taken to obtain 13.1 grams of the salt? B. How many milliliters of 9.95 M hydrochloric acid solution should be used to prepare 4.00 L of 0.300 M HCl? C. Calculate the number of milliters of 0.764 M NaOH required to precipitate as AgOH all of the Ag+ ions in 167 mL of 0.632M AgNO3 solution. D. An aqueous solution of hydrobromic acid is standardized by titration with a 0.169 M solution of barium hydroxide.If 13.0 mL of base are required to neutralize 13.0 mL of the acid, what is the molarity of the hydrobromic acid solution? E. Oxalic acid dihydrate is a solid, diprotic acid that can be used in the laboratory as a primary standard. Its formula is H2C2O4•2H2O.A student dissolves 0.631 grams of H2C2O4•2H2O in water and titrates the resulting solution with a solution of sodium hydroxide of unknown concentration. If 24.1 mL of the sodium hydroxide solution are required to neutralize the acid, what is the…

we can precipitate out solid lead (II) iodide from an aqueous lead(II) nitrate solution by adding potassium iodide. if we have 500. mL of 0.632 M lead(II) nitrate solution how much 1.50 M potassium iodide must we add to exacltly precipitate all the lead (II) ions? 0.211 L 461 mL 0.632 L 0.421 L 0.316 L or 1.19 L

A sample is a mixture of the salts and silver nitrate, copper (II) chloride, and iron (III) chloride. When a 1.000 g sample of the mixture is dissolved in water and reacted with excess silver nitrate, 1.7809 g of precipitate forms. When a separate 1.000g sample of the mixture is treated with a reducing agent, all the metal ions in the sample are reduced to pure metals. The total mass of the metals produced is 0.4684g. Calculate the percent of each salt in the original mixture.