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(a)
Interpretation:
The decreases of solubility of
Concept introduction:
The solubility of compounds depends on pH of solution. Also, the solubility of compound such as oxide and strong base is dependent on pH.
The pH of ionic compound is inversely proportional to solubility. The solubility of salt that has basic anion will increase. If strong acid is added to solution, the concentration of anion decrease which decreases the magnitude of ion form.
In accordance to Le Chatelier’s principle, acidic pH increases the solubility of salt that has anion is conjugate base of weak acid. Also, pH has no effect on the solubility of salt that has anion of conjugate base of strong acid.
(b)
Interpretation:
The increase of solubility of
Concept introduction:
The solubility of compounds depends on pH of solution. Also, the solubility of compound such as oxide and strong base is dependent on pH.
The pH of ionic compound is inversely proportional to solubility. The solubility of salt that has basic anion will increase. If strong acid is added to solution, the concentration of anion decrease which decreases the magnitude of ion form.
In accordance to Le Chatelier’s principle, acidic pH increases the solubility of salt that has anion is conjugate base of weak acid. Also, pH has no effect on the solubility of salt that has anion of conjugate base of strong acid.
(c)
Interpretation:
The decrease of solubility of
Concept introduction:
The solubility of compounds depends on pH of solution. Also, the solubility of compound such as oxide and strong base is dependent on pH.
The pH of ionic compound is inversely proportional to solubility. The solubility of salt that has basic anion will increase. If strong acid is added to solution, the concentration of anion decrease which decreases the magnitude of ion form.
In accordance to Le Chatelier’s principle, acidic pH increases the solubility of salt that has anion is conjugate base of weak acid. Also, pH has no effect on the solubility of salt that has anion of conjugate base of strong acid.
d)
Interpretation:
The increase of solubility of
Concept introduction:
The solubility of compounds depends on pH of solution. Also, the solubility of compound such as oxide and strong base is dependent on pH.
The pH of ionic compound is inversely proportional to solubility. The solubility of salt that has basic anion will increase. If strong acid is added to solution, the concentration of anion decrease which decreases the magnitude of ion form.
In accordance to Le Chatelier’s principle, acidic pH increases the solubility of salt that has anion is conjugate base of weak acid. Also, pH has no effect on the solubility of salt that has anion of conjugate base of strong acid.
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Chapter 17 Solutions
Chemistry, Loose-leaf Edition (8th Edition)
- The equilibrium constant, Kc , for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) is 6.90 x 103 . (a) What is Kc for the reaction 2 SO3 (g) → 2 SO2 (g) + O2 (g) (b) What is Kc for the reaction SO2 (g) + 1/2 O2 (g) → SO3 (g)arrow_forwardThe equilibrium constant for the reaction N,O,(2) = 2NO,(8) is 6.10 x 10 ' at 25'C. Calculate the value of K for this reaction: NO,(g) = 1/2N,O4(g) (A) 327 (B) 164 (C) 12.8 (D) 3.05 × 10 ³ How many moles of HCOON must be added to 1.0 L of 0.10 M HCOOH to prepare a buffer solution with a pH of 3.4? (HCOOH K, = 2 × 10 “) (A) 0.01 (B) 0.05 (C) 0.1 (D) 0.2 What is the percent ionization of a 0.10 M solution of formic acid at 25°C? Formic acid, HCOOH, has a Ka value of 1.9 x 104 at 25°C. (A) 0.19% (B) 1.4% (C) 4.4% (D) 14%arrow_forwardCalculate the maximum concentration of silver ion (Ag+) in a solution that contains 0.025 M CO32–. The compound Ag2CO3 has Ksp= 8.1 x 10–12. (A) 3.2 x 10–10 M (B) 1.6 x 10–10 M (C) 1.8 x 10–5 M (D) 3.6 x 10–5 Marrow_forward
- CH4(g) + 2 HS(g) = CS, (g) + 4 Ha(g) A reaction mixture initially contains 0.50 M CH, and 0.75 M HS. If the equilibrium concentration of H, is 0.44 M, find the equilibrium constant (K) for the reaction.arrow_forwardWhat is the molar concentration of K + in a solution that contains 63.3ppm of K 3 Fe(CN) 6 ?arrow_forwardWhat volume (mL) of 0.0.214 M (NH4)2HPO4 is necessary to precipitate the calcium as Ca3(PO4)2 from 838 mg of a sample that contains 9.74% Ca?arrow_forward
- Write the equilibrium constant for C(s) + 2H2(g) ↔ CH4(g)arrow_forwardA buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solutionto prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10–4 a.Calculate the pH of the buffer solution. [2]b.What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH hasbeen added to only 100.0 cm3 of this bufferarrow_forwardWhat is the molar concentration of all the ions in a solution of 0.120M Al2(SO4)3?arrow_forward
- The reaction 2CO(g) + O2(g) = 2 CO2(g) is known to be exothermic. According to Le Chatelier's principle, how will this reaction's equilibrium be affected if the reaction temperature is increased? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will increase and the reaction will shift to the right. (D) The equilibrium constant will be unchanged, but the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.arrow_forwardSuppose that the equilibrium constant for chemical reaction 2A><B is 2.3 x 10^7, what is the equilibrium constant for the reaction B><2Aarrow_forwardNickel sulfate, NiSO 4 , reacts with sodium phosphate, Na 3 PO 4 , to give a pale yellow-greenprecipitate of nickel phosphate, Ni 3 (PO 4 ) 2 , and a solution of sodium sulfate, Na 2 SO 4.. How manymilliliters of 0.375 M N i SO 4 will react with 45.7 mL of 0.265 M Na 3 PO 4 ? . Show balanced chemicalreaction of the problem.arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
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