Succinic acid is a diprotic acid with formula of HOOCCH2CH2COOH which we can represent as H2R. Suppose a 100.00-mL solution of 0.1000M Na2R is titrated with 0.2000M HCl.
Ka1 for Succinic acid = 6.21 x 10^-5
Ka2 = 2.22 x 10^-8
1. What is the pH after addition of 75.00 mL of 0.2000M HCl to the Na2R solution?
2. What is the pH after addition of 100.00 mL of 0.2000 M HCl to the Na2R solution?
Succinic acid is a diprotic acid with formula of HOOCCH2CH2COOH which we can represent as H2R....
Tartaric acid is a diprotic acid we can represent as H2T. Suppose a 100mL solution, which contains 0.1000M T2- is titrated with 0.2000M HCl. Ka1=6.21x10-5 and Ka2 = 2.22x10-8. a) What is the initial pH of the T2- above? (before any HCl is added) b) What is the pH after the addition of 100mL of 0.2000M HCl to the T2- above? Please show all work!
Succinic acid (H2C4H6O4), which we will denote H2Suc, is a biologically relevant diprotic acid with the structure shown below он он о нн Q Tap image to zoom . It is closely related to tartaric acid and malic acid. At 25°C the acid-dissociation constants for succinic acid are Kai-6.9 10-5 and Ka2-2.5 x 10-6 Part A Determine the pH of a 0.37 M solution of H2Suc at 25 C, assuming that only the first dissociation is relevant. Express your answer...
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2? 6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
Part A.) Consider that you are titrating a diprotic weak base "B" which has pKb1=4 and pKb2=8. The product of the first ionization of B is BH+ and the product of the second ionization is BH22+. A 0.00500-mol sample of the base is dissolved in enough water to produce 100.0 mL of solution and is titrated with 0.500 M HCl. What is the exact pH when 7.2 mL of HCl is added? Enter your answer to three significant figures. Part...
Acid/Base titrations 10. 25.0 mL of 0.100 M H2A (a weak diprotic acid) is titrated with 0.200 M NaOH. What is the pH of the solution when 0.00 mL, 10.0 mL, 12.5 mL, 20.0 mL, 25.0 mL, and 40.0 mL E.S RaWeMA 5.83 x 10 8) have been added? (Ka1= 2.46 x 10, Ka2 ANSWER: 0 mL = 2.315, 10.0 mL= 4.211 (or 4.213), 12.5 mL = 5.422, 20.0 mL 7.410, 25.0 mL = 9.966, 40.0 mL = 12.664 11....
Calculate the pH of each solution. A solution containing 0.0320 M maleic acid and 0.046 M disodium maleate. The Ka values for maleic acid are 1.20 x 10 (Ka1) and 5.37 x 10-7 (Ka2) 1.8 pH A solution containing 0.0306 M succinic acid and 0.019 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 x 105 (Kal) and 2.31 x 10 (Ka2) pH
Calculate the pH of each solution. A solution containing 0.0345 M0.0345 M maleic acid and 0.047 M0.047 M disodium maleate. The ?aKa values for maleic acid are 1.20×10−2 (?a1)1.20×10−2 (Ka1) and 5.37×10−7 (?a2).5.37×10−7 (Ka2). pH= A solution containing 0.0320 M0.0320 M succinic acid and 0.018 M0.018 M potassium hydrogen succinate. The ?aKa values for succinic acid are 6.21×10−5 (?a1)6.21×10−5 (Ka1) and 2.31×10−6 (?a2).2.31×10−6 (Ka2). pH=
Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11. What is the pH of a 0.47 M solution of carbonic acid?
Solving for the pH in a mixture of acids is like dealing with a diprotic acid. You solve the problem by dealing with the acids in successive order. You start with the stronger acid (just like you start with the Ka1 because it is higher than the Ka2 for a diprotic). Afterward, you move on to the weaker acid. If a solution contains 0.014 M HCl and 0.100 M HF (Ka=6.6x10-4), what will be the pH of the solution?
Solving for the pH in a mixture of acids is like dealing with a diprotic acid. You solve the problem by dealing with the acids in successive order. You start with the stronger acid (just like you start with the Ka1 because it is higher than the Ka2 for a diprotic). Afterward, you move on to the weaker acid. If a solution contains 0.038 M HCl and 0.100 M HF (Ka=6.6x10-4), what will be the pH of the solution?