Question

References Mailings Review View 1) A bottle on the shelf is labeled 0.125 M HNO, (HNO, has a molar mass of 63.02 g/mol) (a) of measure out 30.0 mL of that solution, what mass of HNO, does it contain? (b) What volume of that solution should I measure if I have a reaction that requires 0.0620 mol of HNO3? 2) If I dissolve 10.0g of sodium phosphate, Na PO: (molar mass 163.95 g/mol), in a total volume of 500.0 mL of water what is the concentration (in mol/L) of (a) sodium phosphate (b) phosphate anions (c) sodium cations (d) I take 10.0 mL of the solution in question 2) and dilute it to a new volume of 200.0 mL with water. What is the new concentration of sodium phosphate (in moll)? (e) Write a chemical equation representing what happens to sodium phosphate, Na PO when it goes into solution 3) All the following compounds are soluble in water. Indicate if a solution of them would be a strong electrolyte, a weak electrolyte or a non-electrolyte Calcium nitrate, Ca(NO3)2 Potassium hydroxide, KOH Focus MacBook Air

Answer 1

aAs per guidelines,answer for Q 1 is given here.

- 1 a) Given molarity of HNO3 = 0.125 m. Mass of H Noz corresponding to 30 mL of the solution 0.125 mol x 63.02 g not x 30 xl x 16 1000 WL : 0.125 x 63.02* 30 g 100 0.125*63.02 X 0.03 g. = - 0.2363 g, ... mass of HNO3 = 0.2363 8. b) Amount of HNO3 = Molarity & volume. Given amount of H NUR = 0.0620 mol. * Molarity of HNO3 = 0.125 M. .: Volume = Amount of it NO3 = 0.0620 mol of HNO3 Molarity 0.125 hei/L = 0.4914 = 0.496X1000mL = 496 mL