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Ch.17 - Aqueous Ionic Equilibrium
All textbooksTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblem 125
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Chapter 17, Problem 125

If a hard water solution is saturated with calcium carbonate, what volume of the solution has to evaporate to deposit 1.00 × 10^2 mg of CaCO3, given that one of the main components of hard water is CaCO3, and when hard water evaporates, some of the CaCO3 is left behind as a white mineral deposit?

Verified step by step guidance
1
Identify the molar mass of calcium carbonate (CaCO_3) by adding the atomic masses of calcium (Ca), carbon (C), and oxygen (O).
Convert the mass of CaCO_3 (1.00 \times 10^2 \text{ mg}) to grams by dividing by 1000.
Calculate the number of moles of CaCO_3 using the formula: \text{moles} = \frac{\text{mass in grams}}{\text{molar mass}}.
Determine the concentration of CaCO_3 in the saturated solution, which is typically given or can be found in a reference table.
Use the concentration to find the volume of solution needed to contain the calculated moles of CaCO_3, using the formula: \text{volume} = \frac{\text{moles}}{\text{concentration}}.
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Related Practice
Textbook Question

A 5.55-g sample of a weak acid with Ka = 1.3⨉10-4 was combined with 5.00 mL of 6.00 M NaOH, and the resulting solution was diluted to 750.0 mL. The measured pH of the solution was 4.25. What is the molar mass of the weak acid?

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Open Question
From the data given—where a 0.552-g sample of ascorbic acid (vitamin C) is dissolved in water to a total volume of 20.0 mL and titrated with 0.1103 M KOH, the equivalence point occurred at 28.42 mL, and the pH of the solution at 10.0 mL of added base was 3.72—determine the molar mass and dissociation constant (Ka) for vitamin C.
Open Question
Calculate the pH at the beginning of the titration, at the equivalence point, at one-half of the equivalence point, and at 5.0 mL beyond the equivalence point to sketch the titration curve from Problem 123. Then, choose a suitable indicator for this titration from Table 17.1.
Open Question
If the sodium concentration in blood plasma is 0.140 M, and Ksp for sodium urate is 5.76 * 10^-8, what minimum concentration of urate would result in precipitation?
Textbook Question

Pseudogout, a condition with symptoms similar to those of gout (see Problem 126), is caused by the formation of calcium diphosphate (Ca2P2O7) crystals within tendons, cartilage, and ligaments. Calcium diphosphate will precipitate out of blood plasma when diphosphate levels become abnormally high. If the calcium concentration in blood plasma is 9.2 mg/dL, and Ksp for calcium diphosphate is 8.64⨉10-13, what minimum concentration of diphosphate results in precipitation?

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Textbook Question

Calculate the solubility of silver chloride in a solution that is 0.100 M in NH3.

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