When 35 mL of 0.15 M lead nitrate solution is mixed with 20 mL of 0.12 M chromic sulphate solution, ....... `xx10^(-5)` moles of lead sulphate precipitate out. (Round off to the Nearest Integer).

On mixing 45.0 mL of 0.25 M lead nitrate solution with 25.0 mL of 0.10 M chromic sulphate solution, precipitation of lead sulphate are formed? Also calculate the molar concentration of the species left behind solution. Assume the lead sulphate is completely insoluble.

Upon mixing 50.0 mL of 0.1 M lead nitrate solution with 50.0 mL of 0.05 M chromic sulphate solution, precipitation of lead sulphate takes place. How many moles of lead sulphate are formed and what is the molar concertration of chromic suplhate left in the solution?

Upon mixing 50.0 mL of 0.1 M lead nitrate solution with 50.0 mL of 0.05 M chromic sulphate solution, precipitation of lead sulphate takes place. How many moles of lead sulphate are formed? Also, calculate the molar concentration of the species left behind in the final solution. Which is the limiting reagent?

20 mL of 0.5 M HCl is mixed with 30 mL of 0.3 M HCl, the molarity of the resulting solution is :

100 ml of 0.15 M HCl is mixed with 100 ml of 0.05 M HCl, is the pH of the resulting solution?

Find the volume of 0.1 M potassium dichromate solution required to oxidise 20 ml of 0.6 M ferrous sulphate solution in acid medium