A 27 mL sample of 0.100 M oxalic acid (Ka1= 5.60 * 10^-2, Ka2= 5.42* 10^-5) was titrated with 0.0850 M NaOH.
What is the pH at 4 mL before the equivalence point?
What is the pH at 4 mL after the equivalence point?
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A 27 mL sample of 0.100 M oxalic acid (Ka1= 5.60 * 10^-2, Ka2= 5.42* 10^-5)...
A 27 mL sample of 0.100 M oxalic acid (Ka1= 5.60 * 10^-2, Ka2= 5.42* 10^-5) was titrated with 0.0850 M NaOH. What is the pH at 4 mL before the equivalence point? What is the pH at 4 mL after the equivalence point?
A 0.100 M oxalic acid, HO2CCO2H, solution is titrated with 0.100 M KOH. Calculate the pHs when 25.00 mL of oxalic acid solution is titrated with 10, 15, 20, 25, 35, 40, 45, 50 and 55 mL of NaOH. Kal = 5.4 x 10-2 and Ka2 = 5.42 x 10-5 for oxalic acid. Show all your work and make a graph of pH versus Vb
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
а он (15 points) A 0.100 M oxalic acid, HO,CCOH, solution is titrated with 0.100 M KOH. Calculate the pHs when 25.00 mL of oxalic acid solution is titrated with 10, 15, 20, 25, 35, 40, 45, 50 and 55 mL of Nont Kal = 5.4 x 10-2 and K 2 = 5.42 x 10- for oxalic acid. Show all your work and make a graph of pH versus Vo HO, CCO 2H + KOH KC204 + H2Oenwot aunt men...
A sample of 0.100 M acetic acid (Ka = 1.8 × 10−5) in 50.0 mL of solution is titrated with standard 0.100 M NaOH. What is the pH in the titration flask after addition of 15.0 mL of NaOH?
calculate the pH and pOH for a 0.15 M oxalic acid H2C2O4 solution. (ka1-6.0x10^-2, Ka2-6.1x10^-5)
Calculate the pH of 1.00 x 10^-2 M oxalic acid solution. Calculate the pH of 1 x 10^-2 M solution of sodium oxalate. Ka1 = 5.62 x 10^-2, Ka2 = 5.42 x 10^-5
A 150 mL sample of a 0.300 M solution of K2SO3 is titrated with a 1.00 M HCl solution. Ka1=1.39E10^-2, Ka2=6.73E10^-8 What is the initial pH (before titration) and the pH after 50.0 mL of the 1.00 M HCl has been added?
A sample of 0.100 M acetic acid (K, - 18*10*5) in 300 ml. of solution is titrated with standard 0.100 M NaOH. What is the pH in the titration flask after addition of 15.0 ml. of NaOH? 02.18 On30 Oct. oo Od 11.40 De 47
Consider a the titration of 2.5 M sulfurous acid (H2SO3, Ka1 = 1.5e-2, Ka2 = 1.0e-7) with 2.0 M NaOH. What is the pH at the first halfway point of the titration? What is the pH at the second halfway point of the titration? What is the pH at the equivalence point of the titration?