Q1:
(a) Cu2+(aq) + 4 Cl- [CuCl4]2-
(b) CuCO3 precipitate will form .
(c)
[CuCl4]2- + CO32- CuCO3 + 4 Cl- K = (1/Kf)×(1/Ksp) = 1/(2.5×10-10×5×105) = 105/12.5 = 8.0×103
Q2:
(a) F-(aq) + H2O HF + OH-
(b) weak acid HF is produced .
(c) the solution would be basic .
Because KF is a salt of strong base and weak acid, anionic hydrolysis would releases OH- ions .
1. A complex, [CuCl 5.0x10 forms when mixing aqueous solutions of CuCla and NaCl. The Kr...
multi photo exp # on last photo Acid-Base Properties of Salt Solutions Worksheet 1. What is a salt? How is it formed? 2. What is pK, and what does it represent? How does this value correspond to the strength of an acid? 3. What is pK, and what does it represent? How does this value correspond to the strength of a base? 4. How is pH affected by the concentration of a solution? 5. What does Kw represent? How is...
0.1 molar NaCl solution Identify the acid and base which reacted to form NaCl. Identify each as strong or weak. Acid: __________________ Strength:_________ Base: __________________ Strength:_________ Calculate the theoretical pH of the solution. Show your work. If appropriate, write out the hydrolysis reaction equation. . Measure the pH of the aqueous solution and determine the experimental Kh. pH of solution: _________ Experimental Kh: ____________ a) How does the theoretical pH correspond to the experimental pH? b) List two factors which...
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...
61.8% Tools F 8. Sign 0.1 molar NH4Cl solution 20. Identify the acid and base which reacted to form NH CI Identify each as strong or weak. Acid: Strength: Base: Strength 21. Calculate the theoretical pH of the solution. Show your work. If appropriate, write out the hydrolysis reaction equation. 22. Calculate the theoretical Kh value. 23. Measure the pH of the aqueous solution and determine the expenmental K. Show your work. pH of solution Experimental K. 24. How does...
Please help with the blank starred problems!! if more info needs to be given, please tell me what else you'd need because I don't know. VOOL Data report sheet. Name Desk # Room # Box 3. Weak base: data and calculations Measurements (a) Volume of weak base stock solution diluted 11.60mL 700 (b) Concentration of weak base stock solution = 0.100M (c) Concentration of weak base after dilution - find (d) Weak base measured pH : trial I - 10:41...
1. Predict the precipitate that forms when aqueous solutions of barium chloride and potassium sulfate are mixed? Write the overall and net ionic equation. Identify the spectator ions. 2. Write the balanced equation and the net ionic equation for the reaction of aluminum with hydrobromic acid? Determine which species is oxidized and which is reduced, as well as the oxidizing and reducing agents.
1. A precipitate forms when aqueous solutions of copper(II) iodide and silver(I) nitrate are combined. 2. A precipitate forms when aqueous solutions of copper(II) iodide and sodium hydroxide are combined. 3. Consider the reaction when aqueous solutions of barium bromide and potassium sulfate are combined. The net ionic equation for this reaction is: 4. Consider the reaction when aqueous solutions of barium sulfide and calcium bromide are combined. The net ionic equation for this reaction is: 5. Write a net...
In a preparation of a buffer, 1.0 L of weak acid solution of phenol HOC6H5 with [M] = 0.85 M was mixed with its phenolic salt NaOC6H5 of [M] = 0.80 M. (Ka for HOC6H5 = 1.6 X 10-10) (i)Write equilibrium chemical equation for ionization of HOC6H5 ? (ii)Write equilibrium chemical equation for hydrolysis of the anion OC6H5 ? (iii)Calculate the pH of this solution using the Henderson-Hasselbalch equation? (iv)(a)Calculate the pH after 50 mL of 1.5 M HCl has...
1) When a weak acid is neutralized by a strong base, is the neutralization complete? Write the neutralization reaction for HF and KOH. What is the value of Kn (equilibrium constant for neutralization)? (Ka(HF)=3.5*10^-4). If stoichiometric amounts of acid and base are reacted will the resulting solution be acidic, basic, or neutral? Answer: Kn= 3.5*10^10; neutralization reaction is 100% complete since Kn is so large; pH > 7 at equivalence. Just need this explained please :)
I need help with these problems 07 Question (12 points) e See page 816 1st attempt See Hint Part 1 (6 points) Calculate the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H20. Ksp = 3.50x10-16 at a specifictemperature. See Hint Part 2 (6 points) What is the pH of this solution of cobalt(II) hydroxide? pH 04 Question |See page 792 (15 points) A buffer solution includes a weak acid and its conjugate base. 1st attempt See Hint Feedback Include...