The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO 4 , 0.0118 g/100 mL. (b) Ba ( BrO 3 ) 2 ⋅ H 2 O , 0.30 g/100 mL. (c) NH 4 MgAsO 4 ⋅ 6H 2 O , 0.033 g/100 mL. (d) La 2 (MoO 4 ) 3 , 0.00179 g/100 mL
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO 4 , 0.0118 g/100 mL. (b) Ba ( BrO 3 ) 2 ⋅ H 2 O , 0.30 g/100 mL. (c) NH 4 MgAsO 4 ⋅ 6H 2 O , 0.033 g/100 mL. (d) La 2 (MoO 4 ) 3 , 0.00179 g/100 mL
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.
Consider an analyte solution of 50.0mL of 0.050M hydrochloric acid, HCl, titrated against
0.10 M sodium hydroxide, NaOH (the titration you will be performing in the lab!).
(a) What is the chemical equation representing the titration reaction?
(b) At the start of the titration, before any NaOH is added, what ions or molecules are present in the solution? You only need to list chemical species that are present in appreciable quantities - anything that is considered a small enough concentration to where you’d make a small-change approximation on an ICE table doesn’t need to be included.
(c) Which of species you identified in part (b) will determine the pH of the solution?
(d) After adding 12.50mL of the NaOH, halfway to the equivalence point, what ions or molecules are present in the solution?
(e) At the equivalence point, after adding 25.00mL of NaOH, what ions or molecules are present in the solution?
(f) Which of the species you identified in part (e) will determine…
7.
The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq).
(Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq)
Determine whether each of the following statements concerning this titration is true or false.
(A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3
(B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration
(C) Phenolphthalein would be a suitable indicator for both titrations
Group of answer choices
a.) A) False B) True C) True
b.) A) False B) False C) True
c.) A) False B) True C) False
d.) A) True B)True C)True
6. A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.150 M acetic acid (CH3COOH) solution.
(A) write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer.
(B) Write the complete ionic equation for the reaction that occurs when few drops of sodium hydroxide solution are added to the buffer.
Group of answer choices
a.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq)
(B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l)
b.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq)
(B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq)
c.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq)
(B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l)
d.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq)
(B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq)
General, Organic, and Biological Chemistry (3rd Edition)
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