If 18.7 ml of 0.800 m hcl solution are needed to neutralize 5.00 ml of a household ammonia solution, what is the molar concentration of the ammonia? nh3(aq) + hcl(aq) →nh4cl(aq)

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27-09-2017
Chemistry

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If 18.7 ml of 0.800 m hcl solution are needed to neutralize 5.00 ml of a household ammonia solution, what is the molar concentration of the ammonia? nh3(aq) + hcl(aq) →nh4cl(aq)

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W0lf93 W0lf93 · Answer 1 · 2017-10-07T15:04:24+02:00

2.99 m Looking at the balanced equation, it takes 1 mole of HCl to neutralize 1 mole of NH3. So you can multiply the volume of both reactants by their molarity and set them equal to each other. The expression is 18.7 * 0.800 = 5.00 * x And solve for x. 14.96 = 5.00 x 2.992 = x So the molar concentration of the ammonia used is 2.992 m. Since we have 3 significant figures, the result rounded to 3 significant figures is 2.99 m