Phosphoric acid is a triprotic acid in water, ionizing in the following sequential steps: H3PO4+H204H2PO4 +H30+...
17 H3PO4H20S H2PO4 + H30 Phosphoric acid is a triprotic acid in water, ionizing in the following sequential steps: K 7.11 x 103 K6.32 x 108 к, 3 4.5 х 10 13 = H2PO4H20S HPO42- + H30* НРО,- + H20 S PO3-+ H;0* What is the pH ofa 0.20 M H3PO4 solution? A. 2.84 В. 1.46 С. 2.15 D. 4.09 E. 5.37
H3PO4 is a triprotic weak acid. What is the balanced equilibrium defined as Ka2 of H3PO4? O H2PO4 (aq) + H2O(l) =H2O*(aq) +HPO42- (aq) HPO42- (aq) + H2O(1) = OH(aq) + H2PO4 (aq) O HPO42-(aq) + H2O(1) =H20*(aq) + PO43-(aq) O H2PO4 (aq) + H2O(l) = OH" (aq) + H3PO4(aq) O H3PO.(aq) + H2O(1) =H30*(aq) + H2PO4 (aq)
Which of the following is not a conjugate acid-base pair? A H20 and H30+ B. H3PO4 and H2PO4 C. H3PO4 and HPO42- D. HPO42- and PO43 E. H2PO4 and HPO42-
Phosphoric acid is a polyprotic acid (more than one proton that gets ionized) with 3 pK values: pK1=2.15, pK2=6.82 and pK3=12.38. Which molecular species are present at pH 6.82? mostly H3PO4 [H3PO4]=[H2PO4-] mostly [H2PO4-] [H2PO4-]=[HPO42-] mostly [HPO42-] [HPO42-]=[PO43-] mostly [PO43-] There is are no concentrations provided for the question so it is a question on what stage of deprotonation the phosphoric acid is at
Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH, and the concentrations of all species in a 0.500 M phosphoric acid solution. pKa1= 2.16 pKa2 = 7.21 pKa3 = 12.32 What's: H3PO4, H2PO4-, HPO4-2, PO4-3, H+ ,OH- , pH
Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.300 M phosphoric acid solution. pKa1 pKa2 pKa3 2.16 7.21 12.32 [H3PO4]= M [H^+]= M [H2PO4 ^−]= M [OH^−]= M [HPO4 ^2−]= M pH= [PO4 ^3−]= M
What is the pH of a solution of 0.750 M KH2PO4, potassium dihydrogen phosphate? thanks!! At 25 C phosphoric acid, H3PO4, has the following equilibrium constants: H30+ (aq) + H2 PO4 (aq) H30+ (aq) + HP042-(aq) Kal 7.5 x 10-3 Ka2=6.2×10-8 Kas4.2 x 10-13 H, PO4 (aq) + H20(1) H,PO4-(aq) + H2O(1) 근 HPO(a)+H2O()HO (a)P (aq) ▼ Part A At 25 C phosphoric acid, H3PO4, has the following equilibrium constants: H30+ (aq) + H2 PO4 (aq) H30+ (aq) + HP042-(aq)...
Phosphoric acid, H3PO4, is a triprotic acid with the following acid dissociation constants: Ka1 = 7.5 × 10-3 Ka2 = 6.2 × 10-8 Ka3 = 4.2 × 10-13 Which of the following combinations would be best for preparing a pH 7 buffer? a. H3PO4 and NaH2PO4 b. H3PO4 and HCl c. Na2HPO4 and Na3PO4 d. NaH2PO4 and Na2HPO4 e. H3PO4 and Na3PO4
You are instructed to create 400. mL of a 0.39 M phosphate buffer with a pH of 6.2. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. (Enter all numerical answers to three significant figures.) H3PO4(s) + H20(1) =H30+ (aq) + H2PO4 (aq) Kai = 6.9x10-3 H2PO4 (aq) + H20() = H30+(aq) + HPO42- (aq) Ka2 = 6.2x 10-8 HPO42-(aq) + H20(I) = H30+(aq) + PO43-(aq) Ka3 = 4.8 x 10-13 Which of the available chemicals...
You are instructed to create 400. mL of a 0.39 M phosphate buffer with a pH of 6.2. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. (Enter all numerical answers to three significant figures.) H3PO4(s) + H2O(l) = H30+ (aq) + H2P04 (aq) Kai = 6.9 x 10-3 H2PO4 (aq) + H20(1) =H30+ (aq) + HPO42-(aq) Ka2 = 6.2 x 10-8 HPO42-(aq) + H20(I) = H30+(aq) + PO43-(aq) Ka3 = 4.8 x 10-13 Which of...