The ph of 0.1 m kcn solution given pkb cn– 5
WebbThe pH of 0.5 M aqueous NaCN solution is: Class 11. >> Chemistry. >> Equilibrium. >> Ionization of Acids and Bases. >> If pKb for CN^ - at 25^o C is 4.7. The. WebbSo, [H ] = 10–1 M pH = 1. From above equilibrium, 2 × 10–5 = Χ 101 Χ Du –= 2 × 10 4 +[H ] from CH 3 COOH = C = 10–3 –× 2 × 10 4 = 2 × 10–7 M. (C) pH Calculation : Solutions …
The ph of 0.1 m kcn solution given pkb cn– 5
Did you know?
WebbWhich one of the following is a buffer solution? A. 0.40 M HCN and 0.10 KCN B. 0.20 M CH3COOH C. 1.0 M HNO3 and 1.0 M NaNO3 D. 0.10 M KCN E. 0.50 M HCl and 0.10 NaCl ... 5. Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] WebbCalculate the pH of a 0.15 M solution of ammonium bromide. Kb = 1.8 x 10^5 Calculate the pH of ammonia, which has a concentration of H30+=1.0x10^-11M A. 11 B. 2 C. 14 D. 1.0 x 10^-11...
WebbAnswer (1 of 2): As acids go, this is a very weak acid which makes the problem easier as you will see. Remember, that pH = -log [H+] so we have to determine the [H+]. Also, pKa = -log Ka (so Ka = 4.9 * 10^-10) and, for the equilibrium HCN = H+ + CN- Ka = [H+][CN-]/[HCN] So, let [H+] = x, ther... Webb11 juli 2024 · pH=5 HCN rightleftharpoons H^+ + CN^- K_a = [H^+] [CN^-] //[HCN]=10^-10 HCN Initial_(HCN)=1M Delta_(HCN)=-xM Equilibrium_(HCN)=(1-x)M H^+ Initial_(H^+)=0M …
Webb13 apr. 2024 · You have given incomplete data. I'll add that to given section. Answer - pH = 9.2 Explaination - # Given - C = 0.01 M ka(HCN) = 6.2×10^-10 kb(NH3) = 1.6×10^-5 # … WebbFor each compound enter compound name (optional), concentration, volume and Ka/Kb or pKa/pKb values. For example: CH3COOH pKa=4.76 c=0.1 v=10 HCl pKa=-10 c=0.1 v=20 …
WebbCalculate the pH after the addition of 15.0o mL of… A: Initial moles of HClO = Molarity ×Volume = 0.100 M × 40.0 mL = 4mmoles Initial moles of NaOH =… Q: How many grams of NaIO (Kb (IO-)=5x10-4 ; MW=213.9 g/mole) must be added to 40.0 ml of 0.1 M HCl to… A: pOH = pKb + log [NaIO]/ [HOI] pH = 14 - pOH Q: he Ka of acetic acid is 1.8 x 10 -5.
WebbCalculate the pH of a 0.50 M Ba(OH)2 solution. Ba(OH) 2 = Ba 2+ + 2 OH-; soluble hydroxide of alkaline earth metals is a strong base. [OH-] = 2 x 0.50 M = 1.00 M; pOH = … circular air knivesWebbFrom hydrolise of CN-, we have [HCN]= [OH−], so we have: Kb= [HCN] [OH−]/ [CN−]= [OH−] [OH−] (from KOH)/ [CN−]= [OH−]x0.1 M /0.06 M [OH−]≈0.000027 Finally [OH−]= [OH−]+ [OH−]=0.06 M + 0.000027 M =0.060027 M pH=14- (−log [OH−])=14− (-log0.060027)=12.778 Share Improve this answer Follow edited Jun 18, 2024 at 9:15 answered Jun 18, 2024 at … diamond egyptWebbCalculate the pH of a 0.100 M KCN solution. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. diamond eggshell paint 5lWebbWhat will be the pH of 0.1 M CH 3COONH 4? Dissociation constants of CH 3COOH and NH 4OH are K a=1.8×10 −5 and K b=1.8×10 −5 respectively. Medium Solution Verified by Toppr The salt CH 3COONH 4 is formed from weak acid CH 3COOH and weak acid base NH 4OH. CH 3COONH 4+H 2O⇌CH 3COOH+NH 4OH pH= 21pK w− 21pK a− 21pK b diamond electric gastonia ncWebbThe pH of a 0.1 M solution of a weak base is 9.82. What is the Kb for this base? A base will give hydroxide ions in reaction with water. B (aq) + H2O (l) → HB+ (aq) + OH- (aq) From … circular 94 of gstWebb基础化学习题解答_试卷_化学. 创建时间 2024/05/25. 下载量 2 diamond electric danbury ctWebbCalculate the pH of a 0.50 M solution of HCN. K_a for HCN is 4.9 times 10^{-10}. Calculate the pH of a 0.500 M solution of KCN. K_a for HCN is 5.8 times 10^{-10}. HCN is a monoprotic weak acid with a Ka value of 4.90 x 10-10. Calculate the pH of a 7.50 x 10-6 M solution of this acid taking into account the autoprotolysis of water. circular and doubly linked list