Consider the diprotic acid h2a with k1=1.00x10-4 and k2=1.00x10-8. find the pH and concentrations of h2a,...

Consider the diprotic acid h2a with k1=1.00x10-4 and k2=1.00x10-8. find the pH and concentrations of h2a, ha-, and a2- in (a) 0.100 M H2A (b) 0.100 M NaHA (c) 0.100 M Na2A

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queen_honey_blossom answered 1 year ago

Find αH2A for a diprotic acid (H2A) at pH 1.00 (Ka1 = 1.20 × 10-2 &...

Find αH2A for a diprotic acid (H2A) at pH 1.00 (Ka1 = 1.20 × 10-2 & Ka2 = 5.37 × 10-7)

Consider a diprotic acid H2A with ka1=2.510^-6 ka2 2.810^-12 A) what will be the concentrations of...

Consider a diprotic acid H2A with ka1=2.5*10^-6 ka2 2.8*10^-12 A) what will be the concentrations of all species present in a 0.125 M solution of H2A B) what will be the concentrations of all species present in a 0.125 M solution of NaHA

The titration of weak diprotic acid H2A with strong base is conducted. What is the pH...

The titration of weak diprotic acid H2A with strong base is conducted. What is the pH of the solution at the following volumes, 0,10,25,50,60,75,100,125,and 150mL if Ka1=1.0x10^-4 and Ka2=3.5x10^-4 and the concentrations for both HA- and OH- are 0.1M?

The diprotic acid,H2A has two ionizable protons with pKa1=4.175 and pKa2=10.235. Determine the pH, [H2A], [HA-...

The diprotic acid,H2A has two ionizable protons with pKa1=4.175 and pKa2=10.235. Determine the pH, [H2A], [HA- ], [A-2 ], [OH-1 ] for the following three solutions. a) A solution which is 0.1500M in H2A. b) A solution which is 0.1500M in NaA c) A solution which is 0.1500M in Na2A

Glutamine (HQ) is a diprotic amino acid with Ka1=6.5x10^-3 and Ka2=1.00x10^-9. Determine the pH of the...

Glutamine (HQ) is a diprotic amino acid with Ka1=6.5x10^-3 and Ka2=1.00x10^-9. Determine the pH of the following solutions. A) 0.298 M glutamine hydrochloride (H2Q+ Cl-) B) 0.298 M glutamine (HQ) C) 0.298 M sodium glutaminate (Na+Q-)

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 2.40× 10–4 and Ka2 =...

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 2.40× 10–4 and Ka2 = 2.70× 10–12. Calculate the pH and molar concentrations of H2A, HA–, and A2– at equilibrium for each of the solutions below. .185M solution of NaHA .185M solution of Na2A

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 1.63× 10–4 and Ka2 =...

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 1.63× 10–4 and Ka2 = 4.71× 10–11. Calculate the pH and molar concentrations of H2A, HA–, and A2– at equilibrium for each of the solutions below. (a) a 0.184 M solution of H2A (b) a 0.184 M solution of NaHA (c) a 0.184 M solution of Na2A

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.66× 10–4 and Ka2 =...

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.66× 10–4 and Ka2 = 4.99× 10–12. Calculate the pH and molar concentrations of H2A, HA–, and A2– at equilibrium for each of the solutions below. (a) a 0.121 M solution of H2A pH = ? [H2A]=? [HA-]=? [A2-]=? (b) a 0.121 M solution of NaHA pH = ? [H2A]=? [HA-]=? [A2-]=? (c) a 0.121 M solution of Na2A pH = ? [H2A]=? [HA-]=? [A2-]=?

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.94× 10–4 and Ka2 =...

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.94× 10–4 and Ka2 = 2.17× 10–12. Calculate the pH and molar concentrations of H2A, HA–, and A2– at equilibrium for each of the solutions below. (a) a 0.147 M solution of H2A (b) a 0.147 M solution of NaHA

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.61× 10–4 and Ka2 =...

A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.61× 10–4 and Ka2 = 4.02× 10–12. Calculate the pH and molar concentrations of H2A, HA–, and A2– at equilibrium for each of the solutions below. (a) a 0.124 M solution of H2A pH [H2A] [HA-] [A2-] (b) a 0.124 M solution of NaHA pH [H2A] [HA-] [A2-] (c) a 0.124 M solution of Na2A pH [H2A] [HA-] [A2-]

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