![3 Potassum sulite, KSo, contains HSo, which is the anion of the weak polyproticacid sulfurous acid, H250 (a) Write the reactions of this anion acting as a weak acid and as a weak base in water. (i) Reaction as a weak acid: (i) Reaction as a weak base: (b) Use the following information on the Kas of H2SO, below to choose or calculate the correct K for the reactions in (a) K 1.2 x 10 HSO(aq) +H20() HSO, (aq) +HsO (aq) Ko= 66 x 10-8 HSO, (aq) +HO (l)~so,2 (aq) +Hyo. (aq) (i) weak acid, K, (i) weak base, Ko (c) Which of the two reactions in (a) will be the dominant reaction, ( or (i)] ? Which K will dominate? (d) What ions are present in an aqueous solution of 0.123 M KHSO3? (e) Identify the spectator ions, if present. (f) Write the equilibrium K expression for the dominant equilibrium reaction. (8) Calculate the pH of the 0.123 M KHSO>](http://img.homeworklib.com/questions/c560a390-ac47-11eb-9909-079e83997f1c.png?x-oss-process=image/resize,w_560)
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3 Potassum sulite, KSo, contains HSo, which is the anion of the weak polyproticacid sulfurous acid,...
What is the equilibrium constant expression, K i, for the following weak acid? H 2SO 3(...
What is the equilibrium constant expression, K i, for the following weak acid? H 2SO 3( aq) H +( aq) + HSO 3 -( aq) Ki = [H2SO3] / [H+][HSO3-] Ki = [H+]2 [SO32-]/ [H2SO3] Ki = [H+]2 [HSO3-]/ [H2SO3] Ki = [H2SO3] / [H+]2 [SO32-] Ki = [H+][HSO3-]/ [H2SO3
1. For each reaction below Classify each acid, base, conjugate acid, and conjugate base as a...
1. For each reaction below Classify each acid, base, conjugate acid, and conjugate base as a strong acid, weak acid, strong base, or a weak base. Calculate the value of the equilibrium constant II. I. Determine if these reactions need to be treated as an equilibrium (needing an ICE table) or a stoichiometry problem (assuming the reaction goes essentially to completion) a. F-(aq) H2O() HF(aq) + H3O*(aq) + H2O(1) NH3(aq) + b. NH4 (aq) OH (aq) + H3O*(aq) NH3(aq) +...
Writing Proton-Transfer Equations for Acid-Base Reactions •PROBLEM: Write balanced total and net ionic equations for the...
Writing Proton-Transfer Equations for Acid-Base Reactions •PROBLEM: Write balanced total and net ionic equations for the following reactions and use curved arrows to show how the proton transfer occurs. –(a) hydriodic acid (aq) + calcium hydroxide (aq) → Give the name and formula of the salt present when the water evaporates. –(b) potassium hydroxide (aq) + propionic acid (aq) → Note that propionic acid is a weak acid. Be sure to identify the spectator ions in this reaction.
21. The titration of 25.0 ml. of an unknown concentration HSO, solution requires 83.6 ml of...
21. The titration of 25.0 ml. of an unknown concentration HSO, solution requires 83.6 ml of 0.12 M LIOH solution. What is the molarity of the unknown HSO, solution (in MJ? (Write the balanced reaction first) A. 0.20 M B. 0.40 M C. 0.10 M D. 0.36 M E. 0.25 M 22. Complete and balance the following acid-base reaction. What volume of 0.200 M HCI is required for the complete reaction of 1.00 g of Ca(OH): (FW - 74.10g/mol? Ca(OH)(s)...
This question pertains to the pH of a weak acid/weak base salt combo. For an aq...
This question pertains to the pH of a weak acid/weak base salt combo. For an aq solution of NH4NO2, these are the combinations of reactions that are possible. (1) NH4+(aq) + NO21-(aq) ⇆ NH3(aq) + HNO2(aq)____________K1 = ? (2) NH4+(aq) + H2O(l) ⇆ H3O+(aq) + NH3(aq)_______________Ka = 5.6 x 10-10 (3) NO21- + H2O(l) ⇆ HNO2(aq) + OH-(aq)_________________Kb = 2.2 x 10-11 (4) 2H2O(l) ⇆ H3O+(aq) + OH-(aq)_________________________Kw =1.0 x 10-14 Write the symbolic expression for the equilibrium constants...
Answer Strong base is dissolved in 715 ml of 0.400 M weak acid (K. 4.73 x10)...
Answer
Strong base is dissolved in 715 ml of 0.400 M weak acid (K. 4.73 x10) to make a buffer with a pH of 4.05. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) 11,011) +A-(aq) -> Calculate the pka value of the acid and determine the number of moles of acid initially present. Number Number рк,-14.325 0.286mol HA When the reaction is complete, what is the concentration ratio of conjugate base to acid? Number...
the table for problem 5 is attached S. Consider the weak acids in Table 13.2. Which...
the table for problem 5 is attached
S. Consider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of: a) 3.5 b) 7.3 c) 10.0 To make a buffer with pH 3.0 from HCHO2 and CHO2: a) what must the [HCHO2]/[CHO2] ratio be? 6. ep b) how many moles of HCHO2 must be added to a liter of 0.139 M NaCHO2 to give this pH? c) how many grams of NaCHO2...
Strong Acids and [H'] (and pH) The pH of a strong acid is the concentration of...
Strong Acids and [H'] (and pH) The pH of a strong acid is the concentration of the strong acid. 1.OM HCI makes 1.OM H. Except H2SO4. Its pH is a little lower than that because: H2SO4(aq) H+ (aq) + HS07 (aq) Strong acids generally have K.>>1. We assume K = . The HSO, is a weak acid: HSO2 (aq) + H+ (aq) + S0 - Ka = 1.2 * 10-2 Weak Acids and [H+] (and pH) These are weak electrolytes....
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...
please help >< Polyprotic acids have more than one proton to donate to water, therefore have...
please help ><
Polyprotic acids have more than one proton to donate to water, therefore have more than one equilibrium constant for proton donation. For phosphoric acid, there is a three-step equilibrium: H, PO +H,0 5 H2PO4 + H30* H,PO," +H,0 5 HPO - +H30* HPO 2- +,0 5 PO.- +,0* Kai = 7.11 x 10-3 Ka2 = 6.32 x 10-8 Ka; = 4.5 x 10-13 For all conjugate acid base pairs: K, XKK where K is for the reaction...
1. For each reaction below Classify each acid, base, conjugate acid, and conjugate base as a strong acid, weak acid, strong base, or a weak base. Calculate the value of the equilibrium constant II. I. Determine if these reactions need to be treated as an equilibrium (needing an ICE table) or a stoichiometry problem (assuming the reaction goes essentially to completion) a. F-(aq) H2O() HF(aq) + H3O*(aq) + H2O(1) NH3(aq) + b. NH4 (aq) OH (aq) + H3O*(aq) NH3(aq) +...
21. The titration of 25.0 ml. of an unknown concentration HSO, solution requires 83.6 ml of 0.12 M LIOH solution. What is the molarity of the unknown HSO, solution (in MJ? (Write the balanced reaction first) A. 0.20 M B. 0.40 M C. 0.10 M D. 0.36 M E. 0.25 M 22. Complete and balance the following acid-base reaction. What volume of 0.200 M HCI is required for the complete reaction of 1.00 g of Ca(OH): (FW - 74.10g/mol? Ca(OH)(s)...
Answer
Strong base is dissolved in 715 ml of 0.400 M weak acid (K. 4.73 x10) to make a buffer with a pH of 4.05. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) 11,011) +A-(aq) -> Calculate the pka value of the acid and determine the number of moles of acid initially present. Number Number рк,-14.325 0.286mol HA When the reaction is complete, what is the concentration ratio of conjugate base to acid? Number...
the table for problem 5 is attached
S. Consider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of: a) 3.5 b) 7.3 c) 10.0 To make a buffer with pH 3.0 from HCHO2 and CHO2: a) what must the [HCHO2]/[CHO2] ratio be? 6. ep b) how many moles of HCHO2 must be added to a liter of 0.139 M NaCHO2 to give this pH? c) how many grams of NaCHO2...
Strong Acids and [H'] (and pH) The pH of a strong acid is the concentration of the strong acid. 1.OM HCI makes 1.OM H. Except H2SO4. Its pH is a little lower than that because: H2SO4(aq) H+ (aq) + HS07 (aq) Strong acids generally have K.>>1. We assume K = . The HSO, is a weak acid: HSO2 (aq) + H+ (aq) + S0 - Ka = 1.2 * 10-2 Weak Acids and [H+] (and pH) These are weak electrolytes....
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...
please help ><
Polyprotic acids have more than one proton to donate to water, therefore have more than one equilibrium constant for proton donation. For phosphoric acid, there is a three-step equilibrium: H, PO +H,0 5 H2PO4 + H30* H,PO," +H,0 5 HPO - +H30* HPO 2- +,0 5 PO.- +,0* Kai = 7.11 x 10-3 Ka2 = 6.32 x 10-8 Ka; = 4.5 x 10-13 For all conjugate acid base pairs: K, XKK where K is for the reaction...
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