As it forms an amhpoteric salt so its pH = pKa2+pKa3/2=9.75
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2) Calculate the pH of 0.08 M Na2HPO4 H3PO4 S H+ + H2 PO4 pK1 = 2.1 H2PO4 5 H+ + HPO42- pK2 = 7.2 HPO42- 5 H+ PO43- pK3...
3) Calculate the pH of a solution by mixing 50.0 mL of 0.200 M Na2HPO4 with 20.0 mL 0.0400 M NaH2PO4. (Hint: Buffer solution. Use Henderson-Hasselbalch equation) H3PO4 5 H+ + H2PO4 pkı = 2.1 H2PO4 5 H+ + HPO42- pK2 = 7.2 HPO42- 5 H+ PO43- pK3 = 12.3
Calculate the concentrations of all species found in 0.30 M Na2HPO4 solution as well as the pH of this solution: [ For H3PO4 Ka1=7.11x10^-3, Ka2=6.34x10^-8, and Ka3=4.33x10^-13]. a. [Na+] b. [H3PO4] c. [H2PO4] d. [HPO4] e. [PO4] f. [H+] g.[OH-] h. pH=?
Please explain in steps 3.) Calculate the concentrations of all molecular and ionic species and the pH in aqueous solutions that have the following formal compositions: a) 0.05 M acetic acid + 0.1 M sodium acetate; b) 0.2 M boric acid + 0.05 M sodium borate (pK, of boric acid = 9.24); c) 0.5 M hydrochloric acid. Some representative K, and pK, values: Acid Oxalic acid H3PO4 Formic acid Succinic acid Oxalate Acetic acid Succinate H2CO3 H2PO4 NH4+ HCO3 Piperidine...
A. Calculate the pH of a 0.0001 M HNO3 solution B. Calculate the pH of 0.08 M Sr(OH)2 solution C. Calculate the pH of a 0.02 M hydrazoic acid solution (HN3 ----> (H+) + (N3-)), pKa = 4.72 D. Aluminum carbonate (AI2(CO3)3) reacts with phosphoric acid(H3PO4) to produce aluminum phosphate (AIPO4), carbon dioxide, and water 1. Write a balanced equation for the reaction 2. Calculate the mass of phosphoric acid (g) required to react with 100 g of an aluminum...
The following questions is based on ionization of carbonic acid. [H2CO3 = H+ + HCO3- K1 = 4.7 X 10-7, pK1 = 6.34 ] [HCO3- = H+ CO3-2 K2 = 4.4 X 10-11, pK2 = 10.36] Calculate the pH ofthe solution form by mixing the following: a)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.050 M NaOH . b)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.150 M NaOH . c)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.100 M...
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...
please show full work for understanding purposes:) 5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of strontium hydroxide, Sr(OH). Sr(OH)2 = Srz + 20H .0025 - x + x + 2x o rood .0025 - Kb = (2x² 4 = 6.5*103 0.0025 ) pH = 6. (6 pts) Calculate the pH of a 0.175 M NH; aqueous solution. K. for NH, is 1.8 x 10. pH = 180 7. (10 pts) Determine the pH of a...
6. Given a total dissolved lead concentration of 2.0x10-5 M, a total dissolved NTA concentration of 2.0x10-2 M, and a pH of 12.3 (note extreme pH) a. Under these conditions, what is the dominant form of NTA? b. Write an equation for total dissolved NTA and for total dissolved Pb. What assumptions can you make? c. Calculate the predicted [Pb2+], considering NTA complexation only? d. What is the [Pb2+] as predicted by the solubility of Pb(OH)2(s) at pH 12.3? e....
problem 4 magnetic flux through χ-1,0 < y i, i < 2 4. Calculate s Problem 4 (10 points) In free space, A= 10 sinπ ya, + (4 + cosπ x)az wb/m. Find H and J. Problem 5 (10 points) magnetic flux through χ-1,0