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please help!! calculate pH of solutions on second page a-c!! 1. (4 points) A buffer solution...
4, Calculate the [OH1 pH and percent ionization for a 0.2M aqueous solution of NH,. K,- 1.8 x 10 5. Calculate the [H1 and pH of a buffer solution that is 0.10 M CH,COOH and 0.20 M NaCH,COO. 6. How many grams of NH.Cl are needed to 500 mL of a buffer solution that is 0.10 M NH, with a pH of 9.15?
Can anyone please help with how to calculate degree of ionization for the first 3 solutions as well as how to calculate the expected pH for solution 4? thank you! Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
2. Determine the pH of 0.30 M Ba(OH) (aq) (6 points) 3. Determine the pH of 0.20 M Hypoiodous acid, HIO (Ka 23x 10) (8 points) mass of sodium formate, NaHCO, needs to be added to 500.0 ml, 0.100 M formic acid, HCO,H, to produce a buffer solution with a pH of 40 K, (НСОН). 1.8 x 10"İ (8 points)
all please. its okah if its just the answers 18. Calculate the pH of a buffer solution that is 0.410 M in HOCI and 0.050M in NaOCI. [Ka(HOCI) 3.2 x 10* a. 0.39 d. 749 b. 3.94 e) 6.58 19. Which one of these equations represents the reaction of a weak acid with a weak base! a. H'(aq) + OH (aq)- H:O(aq) b. H'(aq)+ CHsNH2(aq)- CHSNH3 (aq) c. OH (aq) + HCN(aq)- H:O(aq) + CN (aq) d) HCN(aq) + CH...
2. A Student wants to prepare 250.0 mL of pH 4.1 buffer solution. He is planning to use formic acid (HCOOH) and sodium formate (HCOONa) for this job. What should the mass of sodium formate that he should add to 250,0 mL of 0.20 M formic acid solution to prepare this buffer? (K =1.8x10 for formic acid.) 3. If 0.10 M solution of a weak acid has a pH of 3.90, find the Ka for the acid.
1. Calculate the pH, pOH and percentage dissociation of a 0.20 M aqueous solution of the weak base, methylamine, CH,NH. The K. for CH,NH, is 3.6 x 10. (partial answer: pH= 11.93) 2. Calculate the pH of 0.75 M (CH3)2N. Ko for (CH3)2N is 7.4 x 10-(Answer pH=11.87) 3. Calculate the pH of 0.10 M NH.NO, K, for NH, is 5.6 x 10-20. (Answer pH=5.13)
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
Calculate the pH at 25 °C of a 0.16 M solution of ethylammonium bromide (C,HNH,Br). Note that ethylamine (C,H,NH) is a weak base with a p K, of 3.19 Round your answer to 1 decimal place. pH X
Buffer Practice 1.) You wish to prepare 750 mL of a buffer solution of pH = 7.00 and you decide to use NaH2PO4 as the acid, K2 = 6.2 x 10. You have on hand a 0.175 M solution of this acid. Kai = 7.5 x 103, Ka2 = 6.2 x 10-8, K3 = 4.2 x 10-13 a.) Calculate the pH of the NaH2PO4 solution. b.) Calculate the grams of Na2HPO4 that need to be added to 750 mL of...
4. (16 Points) A) Calculate the pH of 0.250 Lof a 0.36 M Formic acid HCO2H and 0-30 M Sodium formate, NaCO, buffer. Assume that volume remains constant (K, for HCOH = 1.8 x 10^). B) Calculate the ph of the above buffer after the addition of a) 0.0050 mol of NaOH and b)0.0050 mol of HCI 5. (12 Points) a)Calculate the pH of 100.0 mL 0.20 M NH (K = 1.8 X 105). b)Calculate the pH of a solution...