Homework Answers
The complete step wise calculation is given as below:-
![@ 0.010 M HNO3 So, [ho = [No30 = 0.01m = 102m so, the concentration af [ho] will be [ro] = 102m] since, pH = -log [no] =-log](http://img.homeworklib.com/questions/6b8ea950-7325-11ea-8cf6-13db15a70a65.png?x-oss-process=image/resize,w_560)
![③ we have 0.035 m KOH So [oHo] = [ko] = 0.035m Then por = -log [ona = -log (0.035) om pom = E!)*(-1.456) = 1.456 since, PH +](http://img.homeworklib.com/questions/6c0dc7a0-7325-11ea-9267-ad20ab7c0a54.png?x-oss-process=image/resize,w_560)
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U-3 , cu 6-36. Calculate (H+) and pH for the following solutions:...
2. Calculate the concentrations and activities of H3O+ for the following solutions (assume that the ionic strength...
2. Calculate the concentrations and activities of H3O+ for the following solutions (assume that the ionic strength is determined by the acid/base). Calculate the pH for each solution two ways: 1) pH = -log[H3O+] and 2) pH = -log @,0+. (a) 0.010 M HNO3 (b) 0.035 M KOH (c) 0.030 M HCI (d) 3.0 M HCI
please write out the steps. thanks! 1) Calculate the pH of the following solutions: MHCI kwa...
please write out the steps. thanks!
1) Calculate the pH of the following solutions: MHCI kwa CH] Coir] - loko-14 COH-] = loxio 7 b) 7.0 x 10-5 M NaOH c) 2.0 x 10-6 M HCI d) 3.0 x 10-2 M KOH e) 4.0 x 10-S MHCI
Calculate the pH of the following solutions: a) Calculate the pH of the solution obtained by mixing 20.00 mL of 1.00 M H...
Calculate the pH of the following solutions: a) Calculate the pH of the solution obtained by mixing 20.00 mL of 1.00 M HCl with water until a volume of 2000 mL. b) Calculate the pH by mixing 5.00 mmol of HNO3 with 5.00 mmol of KOH, in a total volume of 1000 mL of solution c) Calculate the pH by mixing 5.00 mmol of C6H5COOH with 3.00 mmol NaOH, and bring up to volume 300 mL. d) Calculate the pH...
2) Calculate the pH of each of the following solutions. a) 0.35 M H2SO4 b) 0.35...
2) Calculate the pH of each of the following solutions. a) 0.35 M H2SO4 b) 0.35 M HCN c) 0.35 M KOH d) 0.35 M CaBr2 e) 0.35 M KCN f) 0.35 M CH3CH2NH2 g) 0.35 M NaHSO4 h) 0.35 M CH3CH2NH3Br
. Calculate the pH of the following solutions: a. 1.00 x 6 M HCI b. 3.25...
. Calculate the pH of the following solutions: a. 1.00 x 6 M HCI b. 3.25 x 104 M HOC c. [OH]-1.0 x 103 10
1. Calculate the pH of the following solutions: (pH = -log (H*]) (a) 0.050 M formic...
1. Calculate the pH of the following solutions: (pH = -log (H*]) (a) 0.050 M formic acid, HCOOH, K=1.78x10-4 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the Ka for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
QUESTIONS 1. Calculate the pH of the following solutions: (pH = -log[H]) (a) 0.050 M formic...
QUESTIONS 1. Calculate the pH of the following solutions: (pH = -log[H]) (a) 0.050 M formic acid, HCOOH. K=1.78x104 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the K, for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
6) Calculate the hydroxide and hydronium ion concentrations for the following solutions a) pH = 7.0...
6) Calculate the hydroxide and hydronium ion concentrations for the following solutions a) pH = 7.0 [H,0") = [OH) = b) pH = 10.00 [H30") = (OH) = 7) From the given value, calculate the other three. Use the figure to take the most efficient pathway possible! a) c) pH = 6.5 PH рона рона [OH-] = [OH") - 1.6 x 10M [H30") - [H,0") - b) d) pH = pH = pOH = 9.8 рон в (OH) = (OH)...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions A) KOH, HNO2 B) H2S03. KHSO3 C) HONH2, HONH3CI D) NaCI, HCI E) RbOH, HF 10) The Henderson-Hasselbalch equation is acid) acid] A) pH- pKa log basel base] D) pH - pKaobase [acid 11) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kp for A- A) A (aq) H30+ (aq) HA (aq) H20 0) B) HA (aq) + OH-(aq) 근...
36) Which one of the following is not a strong acid? (or a weak electrolyte?) a) HNO )HCI HI )HF e) HCIO Answer: 37) The is the conjugate species that remains after an acid donates a proton is ca...
36) Which one of the following is not a strong acid? (or a weak electrolyte?) a) HNO )HCI HI )HF e) HCIO Answer: 37) The is the conjugate species that remains after an acid donates a proton is called its conjugate base. What base of the hydronium ion, HO? B)HO C)HO D)H E HO'has no conjugate base. Answer: acid-base pair? 38) For the reaction shown below, which of the following is a conjugate acid A)CHsN, H:0 B) CsH,N, CsH,NH' C)...
2. Calculate the concentrations and activities of H3O+ for the following solutions (assume that the ionic strength is determined by the acid/base). Calculate the pH for each solution two ways: 1) pH = -log[H3O+] and 2) pH = -log @,0+. (a) 0.010 M HNO3 (b) 0.035 M KOH (c) 0.030 M HCI (d) 3.0 M HCI
please write out the steps. thanks!
1) Calculate the pH of the following solutions: MHCI kwa CH] Coir] - loko-14 COH-] = loxio 7 b) 7.0 x 10-5 M NaOH c) 2.0 x 10-6 M HCI d) 3.0 x 10-2 M KOH e) 4.0 x 10-S MHCI
2) Calculate the pH of each of the following solutions. a) 0.35 M H2SO4 b) 0.35 M HCN c) 0.35 M KOH d) 0.35 M CaBr2 e) 0.35 M KCN f) 0.35 M CH3CH2NH2 g) 0.35 M NaHSO4 h) 0.35 M CH3CH2NH3Br
. Calculate the pH of the following solutions: a. 1.00 x 6 M HCI b. 3.25 x 104 M HOC c. [OH]-1.0 x 103 10
1. Calculate the pH of the following solutions: (pH = -log (H*]) (a) 0.050 M formic acid, HCOOH, K=1.78x10-4 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the Ka for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
QUESTIONS 1. Calculate the pH of the following solutions: (pH = -log[H]) (a) 0.050 M formic acid, HCOOH. K=1.78x104 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the K, for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
6) Calculate the hydroxide and hydronium ion concentrations for the following solutions a) pH = 7.0 [H,0") = [OH) = b) pH = 10.00 [H30") = (OH) = 7) From the given value, calculate the other three. Use the figure to take the most efficient pathway possible! a) c) pH = 6.5 PH рона рона [OH-] = [OH") - 1.6 x 10M [H30") - [H,0") - b) d) pH = pH = pOH = 9.8 рон в (OH) = (OH)...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions A) KOH, HNO2 B) H2S03. KHSO3 C) HONH2, HONH3CI D) NaCI, HCI E) RbOH, HF 10) The Henderson-Hasselbalch equation is acid) acid] A) pH- pKa log basel base] D) pH - pKaobase [acid 11) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kp for A- A) A (aq) H30+ (aq) HA (aq) H20 0) B) HA (aq) + OH-(aq) 근...
36) Which one of the following is not a strong acid? (or a weak electrolyte?) a) HNO )HCI HI )HF e) HCIO Answer: 37) The is the conjugate species that remains after an acid donates a proton is called its conjugate base. What base of the hydronium ion, HO? B)HO C)HO D)H E HO'has no conjugate base. Answer: acid-base pair? 38) For the reaction shown below, which of the following is a conjugate acid A)CHsN, H:0 B) CsH,N, CsH,NH' C)...
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