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1)
Given,
Concentration of CH3COOH solution = 0.15 M
[CH3COOH] = 0.15 M
Concentration of NaCH3COO solution = 0.10 M
[NaCH3COO] = 0.10 M
Acid dissociation constant (Ka) for CH3COOH = 1.8 × 10-5
pH of a buffer solution = ?
Step by step
Solved in 4 steps with 1 images
- Q:3-3 Consider a 1.00 L buffer made by adding 0.140 mol cyanic acid HCNO, and 0.110 mol potassium cyanate ,KCNO, to sufficient water. Calculate the pH a buffer (a) Before any acid or base is added; (b) after the addition of 0.015 mol of HNO3; (c) After the addition of 0.015 mol of KOH. In parts (b) and (c) assume the volume does not change . pka(HCNO)=3.48; ka(HCNO)= 3.3 X 104.A 5.50 g sample of a weak acid with Ka 1.3 x 101 -4 was combined with 5.20 mL of 6.00 M NaOH and the resulting solution was diluted to 750 mL. The measured pH of the solution was 4.15. Part A What is the molar mass of the weak acid? || ΑΣΦ M = 417.93 Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining ? g/molIf a 0.3 M solution of NaOH was used to titrate 100 mL of 0.3 M solution of CH3COOH (Ka =1.8 x 10 -5) and the following volumes of NaOH were recorded: 102, 97, 99, 98, 101, 106 mL. The pH Value is………………when added 99.0 mL of 0.3 M NaOH The pH of the solution at the equivalence point more than 7 Because................................... Calculate the 99% confidence limits of the mean? And use them to decide whether there is any evidence of systematic error? [ hints: For N=6 and the 99 % confidence interval, the value of t is 4.03].
- 1.What is the Ka of a weak acid, HA, that forms a buffer of pH 5.50 when combined in an equal concentration with its conjugate base, A−? Answer: Ka= ...... x 10^-6 2.Calculate the pH of 0.136 M potassium nitrite, KNO2. The ionization constant of nitrous acid, HNO2, is Ka= 5.6× 10-4 3.Calculate the pH of a solution of magnesium hydroxide, Mg(OH)2 (Ksp = 5.6 × 10−12), made by dissolving solid Mg(OH)2 in pure water until the solution is saturated.Edit View History Bookmarks Profiles Tab Window Help 1) * 33% 4 Thu 11:56 AM !! 101 Chem101 PDF A app.101edu.co 山 ☆ Tp ● Update: ΟΥΜΕΝ T | Form.pdf Question 6 of 10 Submit al Determine the pH of a buffer formed by dissolving 21.5 g HC,H,O2 and 37.7 g of NaC,H;O2 in 200.0 mL of solution. The value of Ka for HC,H;O2 is 6.3 x 10-5. ody 2.pdf K PREV 1 2 3 Based on your ICE table and Ka expression, determine the pH of the solution. pH %3D 5 RESET 4.2 x 10-5 6.23 4.37 2.4 x 10 11 7.77 9.63 0.880A 25.0 mL sample of 0.450 M (CH3)2NH is titrated with HBr. What is the pH of the solution after 30.0 mL of 0.375 M HBr have been added to the methylamine solution? ((CH3)2NH; Kb Give answer to 2 decimal places. = 5.9×10-4)
- a) Calculate the pH of a buffer prepared by dissolving 8.00 g of HC7H5O2 and 10.0 g NaC7H5O2 in enough water to make 500. mL of solution. Ka(HC;H5O2) = 1.0 x 10-6 %3D b) What will be the change in pH in the solution in part (a) when 15.0 mL of 1.0 M HCl is added?presented by Macmillan Learning Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K = 6.2 x 10-8, and K3 = 4.8 x 10-13). To find the pH of a buffer composed of H, PO, (aq) and HPO? (aq), which pK, value should be used in the Henderson-Hasselbalch equation? O pKal = 2.16 %3D O PK22 =7.21 O pK33 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH, PO, (s) and 25.0 g of Na, HPO,(s) in water and then diluting to 1.00 L. = Hd Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Scier 7:13 PM 11/8/202 五 0 FZ F8 F10 F11 F12 PrtScr Insert Delete F4 F5 Backspace 23 7. 8. 3. 5. R. E D F H B. N W PgUp Alt Ctrl Home PgDn(а) A student mixed 200 mL of 0.15 M ammonium chloride, NH4CI with 200 mL of 0.23 M ammonia solution, NH3. i) Calculate the pH value of the mixture. 11) Calculate the concentrations of OH in the mixture. [K, for NH3 1.8 x 10 ] (b) Consider a titration between HNO; and NH3, i) write the reaction equation for this titration. ii) sketch the titration curve if the burette contains NH3 and colonical flask contains HNO:. in) classify the salt as neutral, acidic or basic ....Calculate the pH of the buffer solution containing 0.527 M potassium acetate and 0.305 M acetic acid. MМ CH;COOK :98.15 мМ СH,COОH : 60.05 Ka = 1.8x 10-5 CH;COOH CH;COO- + H* Upload your answer and solutions here.SEE MORE QUESTIONS