question 2 please Data Table:Room TemperatureSaturated Solution (25 °C)100 °C Saturated SolutionVolume of saturated,filtered Ca(OH)2 solutionthat was titrated with HCI5.0 mL5.0 mLVolume of HCl solutionConcentration of HCIsolution used in titration required in the titration toreach the equivalence point19.5 mL10.6 mL0.0120 M0.0120 MQuestions/Calculations:1. Based on the titration data (but without really having to do any calculations yet), is the calciumhydroxide more soluble in the room temperature water or the 100 °C temperature water? Explain yourreasoning.2. Calculate the molar solubility and then the Ksp value for Ca(OH)2 at room temperature and 100 °C usingthe titration data.3. Calculate AG for the dissolution of Ca(OH)2 at room temperature and 100 °C.4. Assuming they are constant with temperature, calculate AH° and AS° for the dissolution of calciumhydroxide in water.5. Using the standard thermodynamic values in the Appendix, calculate the theoretical values of AH°, AS°,and AG for the reaction of Ca(OH)2 dissolving in water. Discuss the sign of each and what it tells youabout this reaction.

Given - Volume of Ca(OH)2 at 25°C = 5.0 mL Molarity of HCl at 25°C = 0.0120 M…

Answered: 2. Calculate the molar solubility and…

2. Calculate the molar solubility and then the Ksp value for Ca(OH)2 at room temperature and 100 °C using the titration data.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 12QAP: A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric...

See similar textbooks

Similar questions

A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that volumes are additive. (a) Write a balanced net ionic equation for the reaction that takes place during the titration. (b) What are the species present at the equivalence point? (c) What volume of KOH is required to reach the equivalence point? (d) What is the pH of the solution 1. before any KOH is added? 2. halfway to the equivalence point? 3. at the equivalence point?
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Consider the following pH curves for 100.0 mL of two different acids with the same initial concentration each titrated by 0.10 M NaOH. a. Which plot represents a pH curve of a weak acid, and which plot is for a strong acid? How can you tell? Cite three differences between the plots that help you decide. b. In both cases the pH is relatively constant before the pH changes greatly. Does this mean that at some point in each titration each solution was a buffered solution? c. True or false? The equivalence point volume for each titration is the same. Explain your answer. d. True or false? The pH at the equivalence point for each titration is the same. Explain your answer.
Estimate the solubility of lead(II) bromide (a) in moles per liter and (b) in grams per liter of pure water.
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
How do I calculate the number of moles of potassium permanganate used in each titration?
Calculate the molarity of 25.0 mLof an unknown acid, when it is titrated with 0.2848M NaOH. With its first inlection point at 24.9mL and a second inflection point of 50.2
In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 4: Thymolthalein: pH transition = 8.5-10.5 OIndicator 5: Indigo Carmine: pH transition= 11.6- 14.0 Indicator 3: Cresol red: pH transition 7.2-8.8 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 2: Methyl red: pH transition = 4.8-6.0
A 50.0 mL aliquot of a 0.00100M solution of acetic acid (K, = 1.8 x 10-5) is titrated with 0.00993M NaOH. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration. Properties of Several Indicators Write the letter corresponding to your choice of indicator in the box