What volume of a 0.500 M hydrochloric acid solution is needed to neutralize each

Question

What volume of a 0.500 M hydrochloric acid solution is needed to neutralize each of the following, respectively: a) 10.00 mL 0.300 M sodium hydroxide ; b) 10.00 mL 0.200 M barium hydroxide ?

Explanation / Answer

First, write the balanced equation. NaOH + HCl --> NaCl + H2O 1. Convert 10.00 mL to L. Dividing by 1000, you get 0.01 L. 2. Multiply this by the molarity of NaOH. That way, you'll know how many moles of NaOH was neutralized. 0.01 L * 0.300 mol NaOH / 1 L 3. Then multiply by the mole ratio between NaOH and HCl. The ratio is 1:1. Get it from the coefficients of the balanced equation. 0.01 L * 0.300 mol NaOH / 1 L * 1 mol HCl / 1 mol NaOH = 0.003 mol HCl 4. To solve for the volume of HCl, derive the formula for molarity. M = mol solute / L soln L soln = mol solute / M = 0.003 mol / 0.500 M = 0.006 L

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