Question

Asked Sep 24, 2019

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In the titration of 25.00 mL of a water sample, it took 20.840 mL of 4.350*x* 10^{−3} M EDTA solution to reach the endpoint.

Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures)

**9.07×10 ^{-5}**

The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures)

he total hardness is always listed in parts-per-million (ppm) of CaCO_{3} (or mg CaCO_{3} / Kg H_{2}O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO_{3} per liter of water. Determine the number of moles of CaCO_{3} present in the titrated sample of water, assuming that all the Ca^{2+} combines with CO_{3}^{2−}. (enter your answer with 3 significant figures)

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Step 1

The molarity of a solution is the ratio of number of moles of a substance to the volume of solution in liters. The expression for molarity is labelled in equation (1) in which M is the molarity, n is the number of moles and V is the volume in liters.

The relation between millilitres (mL) and liters (L) is written in equation(2).

Step 2

Convert 20.840 mL in L by using the equation (2) as shown below.

Step 3

The number of moles of EDTA calculated is shown in equation (3) by using equation (...

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