A student prepared a standard copper solution by combining 2.63 mL of stock 0.270 mol/L copper(II) sulfate solution with 6.37 mL of water. What is the molar concentration of Cu2+ in this solution? Give your answer in in decimal format. When entering units, use proper abbreviated units with proper capitalization.

Please help me answer questions 1 and 2. (Questions attached below) 1. When you arrive at the lab, 2.0 M H2SO4(aq) and 2.0 M HC2H3O2(aq) will be present. Youwill need to dilute these solutions using beakers and graduated cylinders from your drawerand DI water.i. Calculate the volume of the 2.0 M HC2H3O2(aq) and DI water needed to create 50.0 mLof 1.05 M HC2H3O2(aq).ii. Calculate the volume of the 2.0 M H2SO4(aq) and DI water needed to create 50.0 mL of0.75 M H2SO4(aq). 2. A 48.33-mL sample of 0.150 M NaBr is titrated into 50.00 mL of 0.145 M AgNO3. Bothsolutions had the same initial and final temperatures. The reaction occurred in a calorimeterwith a known heat capacity and produced 1546.03 J of heat.i. Write a balanced equation that is occurring.ii. Determine the theoretical yield of the solid.iii. Calculate the enthalpy of the reaction (kJ/mole of precipitate).

An analytical chemist weighs out 0.087 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 5.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.

Suppose 0.775 g of sodium iodide is dissolved in 100. mL of a 57.0 m M aqueous solution of silver nitrate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the sodium iodide is dissolved in it. Be sure your answer has the correct number of significant digits.