Homework Answers
(a)
CN- + H2O 
HCN + OH-. Kb =
Kw/Ka
(b)
Al3+ (aq) + H2O
Al(OH)2+ + H+ Ka =
Kw/Kb3
(c)
CO32- + H2O
HCO3- + OH-. Kb =
Kw/Ka2
(d)
CH3COO- + H2O
CH3COOH + OH- Kb =
Kw/Ka
(e)
HCO3- + H2O
H2CO3 + OH- Kb =
Kw/Ka1
HCO3-
H+ + CO32-. Ka1
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CN- (b)Al3+ (c)CO3^2- (d)CH3CO2- HCO3- 3 write a balance equation to show the following ions hydrolyze...
please help with these questions ! 2. Show how methylamine, CH,NH2 dissociates in solution and calculate...
please help with these questions !
2. Show how methylamine, CH,NH2 dissociates in solution and calculate the pH of a 0.25 M aqueous solution of the substance. Kb for CH,NH, is 1.8 x 10-4 3. Write a balanced equation to show how the following ions hydrolyze in water and write the acid or base dissociation constant for each: b) Al3 d0 HCO a) CN CH,СО, c) CO22 d)
Which of the following is not a conjugate acid base pair? a) HCO3-, CO3^2- b) H3O+,...
Which of the following is not a conjugate acid base pair? a) HCO3-, CO3^2- b) H3O+, H2O c) H2PO4-, PO4^3- d) NH3, NH2-
mistake CHM 202 F 19 HW 10 culate the (H). (HSO4)- and ISO 21 - jon...
mistake
CHM 202 F 19 HW 10 culate the (H). (HSO4)- and ISO 21 - jon concentrations and the pH of a 0.050 M H2SO4. Kalis very large and Kis 0.012. 2. Show how methylamine, CH NH dissociates in solution and calculate the pH of a 0.25M aqueous solution of the substance. Ky for CH3NH2 is 1.8 x 10-4 3. Write a balanced equation to show how the following ions hydrolyze in water and write the acid or base dissociation...
B) Given that Ksp of Al(OH)3 is 1.3X10-33, and the following dissociation : Al(OH)3 =→ Al3+...
B) Given that Ksp of Al(OH)3 is 1.3X10-33, and the following dissociation : Al(OH)3 =→ Al3+ + 30H Calculate : 1- The concentration of Al ions in pure water. 2- The pH value of the suspension of Al(OH)3 in water.
Write a balanced net ionic equation to show why the solubility of Zn(CN)2(s) increases in the pre...
Write a balanced net ionic equation to show why the solubility
of Zn(CN)2(s) increases in the presence
of a strong acid and calculate the equilibrium constant for the
reaction of this sparingly soluble salt with acid.
I really need help with both because I am on my last attempt and
cannot seem to understand exactly how to solve for K. Thank you for
your help! I will be sure to rate your answer if it is correct.
Write a balanced...
25. Write the complete equation for the neutralization reactions that take place when the following water...
25. Write the complete equation for the neutralization reactions that take place when the following water solutions are mixed. (If an acid has more than one acidic hydrogen, assume that there is enough base to remove all of them. Assume that there is enough acid to neutralize all of the basic hydroxide ions.) (2 points each) A a. HаРО:(аq) + КОН(аq) b. HCl(aq) +Al2(CO3)s(s)
Calculate and show how you calculated Keq for a, b, and c For each of the...
Calculate and show how you calculated Keq for a, b, and c For each of the following solutions: (i) Enumerate all the possible Brønsted acids and Brønsted bases initially present; (ii) Determine which is the strongest acid and the strongest base; (iii) Write a balanced chemical equation for the reaction between the strongest acid and the strongest base; and (iv) Calculate Keq for this reaction. Use the data provided in the Ka or Kb tables in your textbook as needed....
could someone help me with 15.25 and 15.27 and 15.32 please? $13 Write of the conjugate...
could someone help me with 15.25 and 15.27 and 15.32 please?
$13 Write of the conjugate acid of substances. (The information in Tables 15.6 10/26/2019 the following substances. (The infor and 15.8 may be helpful.) (a) hydrogen sulfate ion (c) ammonia (b) water (d) pyridine he formula and name for the conjugate base of the substances. (The information in Tables 15.6 and 15.24 Writer 15.25 Write the form following substances. (The int 15.8 may be helpful.) (a) nitric acid (b)...
2. (2pts) Write an equation showing mms of hydronium ion concentration. e an equation showing pOH...
2. (2pts) Write an equation showing mms of hydronium ion concentration. e an equation showing pOH in terms of hydroxide ion erms of hydroxide ion concentration 3. Write the dissociation reaction for the following acid symbols. Label the Bronsted-Lowry acid, base, o draw lines to connect the appropriate conjugate pairs: (4 pts) he following acids in water. Use appropriate arrow wry acid, base, conjugate acid, and conjugate base for each, then a. C.H.COOH (benzoic acid) + H2O b. HCI (hydrochloric...
Write an equation for the reaction of each of the following with water a) HNO_3 b)...
Write an equation for the reaction of each of the following with water a) HNO_3 b) HCOOH c) NaOH d) NH_3 (2) Identify the conjugate acid-base pairs in each of the following chemical reactions: a) NH_4^+(aq) + CN^-(aq) NH_3(aq) + HCN(aq) b) CO_3^2-(aq) + HCI(aq) HCO_3^-(aq) + CI^_(aq) c) HCI(aq) + OH^-(aq) H_2O(aq) + CI^-(aq) (3) Classify each of the following as Bronsted acid, Bronsted base, or both in aqueous solution: a) NH_4^+ b) NH_3 c) H_2CO_3 d) HCO_3^- e)...
please help with these questions !
2. Show how methylamine, CH,NH2 dissociates in solution and calculate the pH of a 0.25 M aqueous solution of the substance. Kb for CH,NH, is 1.8 x 10-4 3. Write a balanced equation to show how the following ions hydrolyze in water and write the acid or base dissociation constant for each: b) Al3 d0 HCO a) CN CH,СО, c) CO22 d)
mistake
CHM 202 F 19 HW 10 culate the (H). (HSO4)- and ISO 21 - jon concentrations and the pH of a 0.050 M H2SO4. Kalis very large and Kis 0.012. 2. Show how methylamine, CH NH dissociates in solution and calculate the pH of a 0.25M aqueous solution of the substance. Ky for CH3NH2 is 1.8 x 10-4 3. Write a balanced equation to show how the following ions hydrolyze in water and write the acid or base dissociation...
B) Given that Ksp of Al(OH)3 is 1.3X10-33, and the following dissociation : Al(OH)3 =→ Al3+ + 30H Calculate : 1- The concentration of Al ions in pure water. 2- The pH value of the suspension of Al(OH)3 in water.
Write a balanced net ionic equation to show why the solubility
of Zn(CN)2(s) increases in the presence
of a strong acid and calculate the equilibrium constant for the
reaction of this sparingly soluble salt with acid.
I really need help with both because I am on my last attempt and
cannot seem to understand exactly how to solve for K. Thank you for
your help! I will be sure to rate your answer if it is correct.
Write a balanced...
25. Write the complete equation for the neutralization reactions that take place when the following water solutions are mixed. (If an acid has more than one acidic hydrogen, assume that there is enough base to remove all of them. Assume that there is enough acid to neutralize all of the basic hydroxide ions.) (2 points each) A a. HаРО:(аq) + КОН(аq) b. HCl(aq) +Al2(CO3)s(s)
could someone help me with 15.25 and 15.27 and 15.32 please?
$13 Write of the conjugate acid of substances. (The information in Tables 15.6 10/26/2019 the following substances. (The infor and 15.8 may be helpful.) (a) hydrogen sulfate ion (c) ammonia (b) water (d) pyridine he formula and name for the conjugate base of the substances. (The information in Tables 15.6 and 15.24 Writer 15.25 Write the form following substances. (The int 15.8 may be helpful.) (a) nitric acid (b)...
2. (2pts) Write an equation showing mms of hydronium ion concentration. e an equation showing pOH in terms of hydroxide ion erms of hydroxide ion concentration 3. Write the dissociation reaction for the following acid symbols. Label the Bronsted-Lowry acid, base, o draw lines to connect the appropriate conjugate pairs: (4 pts) he following acids in water. Use appropriate arrow wry acid, base, conjugate acid, and conjugate base for each, then a. C.H.COOH (benzoic acid) + H2O b. HCI (hydrochloric...
Write an equation for the reaction of each of the following with water a) HNO_3 b) HCOOH c) NaOH d) NH_3 (2) Identify the conjugate acid-base pairs in each of the following chemical reactions: a) NH_4^+(aq) + CN^-(aq) NH_3(aq) + HCN(aq) b) CO_3^2-(aq) + HCI(aq) HCO_3^-(aq) + CI^_(aq) c) HCI(aq) + OH^-(aq) H_2O(aq) + CI^-(aq) (3) Classify each of the following as Bronsted acid, Bronsted base, or both in aqueous solution: a) NH_4^+ b) NH_3 c) H_2CO_3 d) HCO_3^- e)...
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