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What volume of 0.0105 -M HBr solution is required to titrate 125 $\mathrm{mL}$ of a $0.0100-M \mathrm{Ca}(\mathrm{OH})_{2}$ solution?$\mathrm{Ca}(\mathrm{OH})_{2}(a q)+2 \mathrm{HBr}(a q) \rightarrow \mathrm{CaBr}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)$

238 $\mathrm{mL}$

00:51

Sisi G.

Chemistry 101

Chapter 4

Stoichiometry of Chemical Reactions

Chemical reactions and Stoichiometry

University of Maryland - University College

University of Kentucky

Brown University

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This is a solution psyche aama tree calculation where we need to balance chemical reaction and we need the concentrations and volumes of the solutions involved. The balanced chemical reaction is one more calcium hydroxide reacts with two moles hydrochloric acid producing one more calcium bromide and two moles of water. So if we have 100 and 25 mil lease milliliters of our calcium hydroxide solution, we can convert it into leaders by dividing by 1000. We can then convert the leaders into moles of calcium hydroxide using the molar itty of the calcium hydroxide solution, 0.1 moles per liter. When we are in units of moles calcium hydroxide, we can use the stock geometry of the balanced chemical reaction to convert into moles of hydroponic acid. Then when we have moles hydroponic acid, we can use the polarity of the hydroponic acid solution to convert the moles hydroponic acid into leaders of the hydroponic acid solution. We do this by dividing by the polarity of the hydroponic acid solution. Then, when we are in units of leaders, we simply multiply by 1000 to get milliliters. So 238 million liters of the 2380.105 molar hydrochloric acid solution are needed to neutralize 125 mL of the 1250.100 moller calcium hydroxide solution.

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