Explain why-(i) Anhydrous calcium chloride is used in desiccators(ii) If bottle full of concentrated H 2SO4 is left open in the atmosphere by accident, the acid starts flowing out the bottle of its own.

Explain why-(i) Anhydrous calcium chloride is used in desiccators(ii) If bottle full of concentrated H 2SO4 is left open in the atmosphere by accident, the acid starts flowing out the bottle of its own.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 91QRT

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In a solution of 0.015 mol L-1 HBr(aq) at 25 °C (a) What are the concentrations of the hydronium, H3O+, and hydroxide, OH-, ions? (Recall that HBr is a strong acid which means it completely ionizes in water ) (b) What is the pH of the solution?
The solubility of Cl, in 100 g of water at STP is 310 cm³. Assume that this quantity of Cl2 is dissolved and equili- brated as follows: Cl2(aq) + H20 = cl (aq) + HCIO(aq) + H*(aq) (a) If the equilibrium constant for this reaction is 4.7 x 10-, calculate the equilibrium concentration of HCIO formed. (b) What is the pH of the final solution?
(a) If the molar solubility of Nd₂(CO3)3 at 25 °C is 1.00e-07 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 8.90e-06 g of Y₂(CO3)3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility- product constant for Y₂(CO3)3. Ksp = (c) The Ksp of Ag₂C₂04 at 25 °C is 5.40e-12. What is the molar solubility of Ag2C₂04? solubility mol/L
(a) If the molar solubility of Sc(OH)3 at 25 °C is 9.52e-09 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 5.73e-05 g of Zn3(ASO4)2 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-product constant for Zn3(ASO4)2. Ksp (c) The Ksp of Nd₂(CO3)3 at 25 °C is 1.08e-33. What is the molar solubility of Nd₂(CO3)3? solubility = mol/L
What is the equilibrium concentration (in M to three decimal places) of NO2 for the following reaction if the initial concentration of N2O4 was 0.250 M?
The powerful oxidizing agent Ce(IV) can be used to quantitatively determine the concentration of methylmalonic acid (MeMA) in a 500 mL beaker. The reaction proceeds as follows: CH3CH(COOH)2 + 6Ce(IV) + 2H₂O → CH3COOH + 6Ce(III) + 6H* + 2CO₂ If the initial concentration of Ce(IV) in the beaker was 0.3M, and 20.0 mL of 0.5 M Fe2+ was required to back-titrate the excess Ce(IV), what was the concentration of Me MA initially present? A. 0.047 M B. 0.28 M C. 0.020 M D. 0.023 M
A chemist wishes to precipitate yttrium cations out of a 1.00 L solution. if the concentration of (in solution is 0.428 M and the K of yttrium iodate is 1.12 x 10, what mass of potassium lodate (00 must be added so that precipitation may begin? The molar mass of potassium lodate is 21A.00 g/mol. (27) (A) (B) (C) (D) 91.6g 64.0 ug (6.4 x 10* g) 411 mg 56.0 ng 137 mg (5.6 x 10* g) (E)
What is the concentration of fluoride ions at equilibrium in a sample of hydrofluoric acid if the initial concentration of hydrofluoric acid is 0.35 M and the Kc is 7.4 x 10-4M?
Hydrogen, a potential fuel, is found in great abundance in water. To separate the hydrogen from the oxygen, water must be thermally decomposed. At 1000°C, the equilibrium constant for this reaction is 7.3 x 10-182H2O(g) + heat <-> 2H2(g) + O2(g) a) If the initial concentration of H2O is 0.350 M, what is the equilibrium concentration of H2? b) Suggest three stresses that could be applied to the equilibrium system to produce more hydrogen.
Why is (CH3)3Cl considered to be a Lewis Acid?
Will a precipitate form if 750.00 mL of a 4.0 x 10-3 mol/L solution of Cerium (III) nitrate, Ce(NO3)3(aq), is mixed in a beaker with 300.00 mL of a 2.0 x 10-2 mol/L solution of potassium iodate, KIO3(aq)?The Ksp for Cerium (III) iodiate, Ce(IO3)3 (s), is 1.9 x 10-10. Justify your answer. n:
Will a precipitate form if 750.00 mL of a 4.0 x 10-3 mol/L solution of Cerium (III) nitrate, Ce(NO3)3(aq), is mixed in a beaker with 300.00 mL of a 2.0 x 10-2 mol/L solution of potassium iodate, KIO3(aq)?The Ksp for Cerium (III) iodiate, Ce(IO3)3 (s), is 1.9 x 10-10. Justify your answer. *There are 6 steps to arrive at the answer. Show all work.Start by writing out a balanced equation for the double displacement equation:

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