a. How many grams of NiSO4 6H₂O are needed to prepare 2.00x10² mL of a 3.5x10² M NISO solution? b. If 15.0 mL of the 3.5x102 M NISO, solution is diluted to 50.0 mL with water, what is the resulting NISO, concentration?

1. If 0.60 mol chlorine reacts with excess sodium, and 1.1 mol NaCl are produced, what is the percent yield for the reaction? 2. We need 35.0 mL of 0.3 M H2SO4 solution to completely titrate 22.00 mL of NaOH solution of unknown concentration.  What is the molarity of the sodium hydroxide solution?          H2SO4  + 2NaOH     Na2SO4   + 2H2O

8. A 200 mL dilute solution of anhydrous CuSO4 with molarity of 0.28 M was made by adding 56 mL of a stock solution, then filling to the 200 mL mark with water. What's the concentration of the original stock solution? M₁ V₁ = M₂ V₂

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…

1. A 500-ml volumetric flask contains 150 ml of 0.200 N H2SO4. By adding a more concentrated H2SO4,  the solution is brought to the mark and after mixing is found to be 0.150 M . What was the normalityof the acid solution?

What is the concentration of HNO3 in the final solution when 70.0 mL of a 6.00 M HNO3 solution is diluted with pure water to a total volume of 0.15L ?

Is this a mole to mole ratio ? If so, what is it ?

A 0.650 ?0.650 m aqueous solution of KBrKBr has a total mass of 86.0 g.86.0 g. What masses of solute and solvent are present?   mass of KBr:                                                      g KBr   mass of water:                                     gH2O     g H2O

a. Calculate the molarity of a solution that contains 0.175 mol ZnCI2 in exactly 150 mL solution. b. How many milliliters of a 6.00 M NaOH solution are needed to provide 0.350 mol of NaOH?

You are given a stock concentration of ADH. The molecular weight of ADH is 35,000 g/mol.  a. What is the molarity of a 54 mg/ml stock solution of ADH? b. you dilute an ADH stock. The concentration is listed below. What is the molarity of a solution made from 78ul of 0 mM stock solution in 17 ml final volume?