scientist is investigating the solubility of two polyatomic ions, oxalate (C2O2−4C2⁢O42−) and arsenate (AsO3−4AsO43−), which are not listed in the table of solubility guidelines. The scientist starts with four solutions made of water-soluble salts. Solution A contains sodium arsenate. Solution B contains ammonium oxalate. Soution C contains silver chlorate. Solution D contains aluminum bromide. Solution Solute

n the laboratory you are given the task of separating Ca2+ and Ag+ ions in aqueous solution.For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. fill in the blank 1 K2SO4   2. fill in the blank 3 HBr   3. fill in the blank 5 Na2CO3

Suppose that you are performing a titration of a hydrochloric acid solution of unknown concentration using a standardized solution of 0.063 M Ca(OH)₂. You prepare the analyte solution by adding 10.0 mL of the unknown hydrochloric acid solution, 40.0 mL of water, and 2 drops of phenolphthalein to an Erlenmeyer flask. You discover that it takes 37.05 mL of Ca(OH)₂ to reach the end point. What is the concentration of the unknown HCl solution? HCl concentration: M

OO HUAWEI P30 LEICA TRIPLE CAMERA a N M

4. A student did not read the directions to the experiment properly and mixed up where to put the NaOH and the HCl solutions. He put the HCl in the buret and the NaOH in the flask. He then added a drop of the phenolphthalein to the solution in the flask. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? Explain qalb ribidw qid edini olddud ris ogrel s znisimos tund entd nousu 5. How many liters of 3.4 M HI will be required to reach the equivalence point with 2.1 L of 2.0 M KOH? 9no vino to beateni nolusius to alsid sigulum ob of insttoqmi ti al VW S

A solution contains Cr3+ and Mg2+. The addition of 1.00 L of 1.53 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 50.0 g . Find the mass of Cr3+ in the original solution.

A 0.430 g sample of a monoprotic acid is dissolved in water and titrated with 0.110 M KOH. What is the molar mass of the acid if 31.0 mL of the KOH solution is required to neutralize the sample? molar mass: g/mol **** -0 -1 2 -3 -4 6 -7 9 10 11 12 13 15 16 17 18 19 20 -21 22 23

A solution contains Cr³+ and Mg2+. The addition of 1.00 L of 1.52 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF₂ (s). The total mass of the precipitate is 49.9 g. Find the mass of Cr³+ in the original solution.

A solution contains 8.85×103 M potassium fluoride and 1.45x102 M ammonium carbonate. Solid lead nitrate is added slowly to this mixture. What is the concentration of carbonate ion when fluoride ion begins to precipitate? [carbonate] = M

Use the References to access important values if needed for this question. The molarity of an aqueous solution of nitric acid, HNO3, is determined by titration with a 9.07 x 10-2 M potassium hydroxide, KOH, solution. HNO3 + KOH → KNO3 + H2O If 39.8 mL of potassium hydroxide are required to neutralize 27.8 mL of the acid, what is the molarity of the nitric acid solution? Molarity = M Submit Answer Retry Entire Group 4 more group attempts remaining