If you need to prepare 500.0 mL of a 0.10 M solution of hydrochloric acid, how m

Question

If you need to prepare 500.0 mL of a 0.10 M solution of hydrochloric acid, how much hydrochloric acid do you need to use? Express your answer in units of moles of HCI needed. Question 13 is a continuation of this question. Moles HCI Calculate the grams of HCI concentrated solution that would be needed to prepare the solution in question 12. The commercially available, concentrated hydrochloric acid solution that would be used for this preparation is 37% (m/m) HCl in water. (Hint: convert moles HCl in question 12 to grams of HCl, then calculate the mass of commercial solution needed to get these grams of HCl)

Explanation / Answer

Q1

we need

Molarity = mol of solute/ Volume of solution (in L)

V = 500 mL

HCl = 0.1 M

mol = MV

mol = (0.1)(0.5) = 0.05 mol of HCl

Q2

mass of HCl

MW of HCl = 36.5 g/mol

mass of HCl = mol*MW = 0.05*36.5 = 1.825 g of HCl required

if 37% required then

1.825/0.37 = 4.932 g of solvent

Total mass = 4.932 g of 37% is required

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