Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
The Ka of a monoprotic weak acid is 4.25 x 103. What is the percent ionization of a 0.153 M solution of this acid? Number
If the equilibrium constant for the acid dissociation is KA and pKA (-log Ka) =7.0, what is the ratio of [HPO42-] to [H2PO4−] in this buffer system? Please show your calculation.
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A. 2x 10-14 В. -log Ka C. pH 7 D. hydrogen ion donor рн E. water F. hydrogen ion acceptor рКа G. H30 OH т рКw H. -log [OH Concentration of [OH] in pure water 1. Ка т Кw Bronsted acid J.1 x 107 M Bronsted base К. 14 L. pH 7 Can act as both an acid and a base М. Кь N. 1 x 1014 O. -log [H30*] Р. рн <7
A buffer solution with a pH of 4.25 is prepared with the same volumes of _________ M formic acid and 0.12 M sodium formate. The Ka of formic acid is 1.8 ⋅ 10-4. 3.7×10−2 0.38 1.8×104 7.5×10−2 1.9×10−2
which of the following would be a correct definition for pKa -the inverse log (1/log value of the Ka -the pH of the acidic solution when the acidic form has been completely converted to its conjugate base form
A benzoic acid/potassium benzoate buffer solution has a pH = 4.25. The concentration of benzoic acid (C6H5COOH, Ka = 6.5 × 10-5) in the solution is 0.54 M. What is the concentration of potassium benzoate (KC6H5COO, Kb = 1.5 × 10-10) in this buffer solution?
A benzoic acid/potassium benzoate buffer solution has a pH = 4.25. The concentration of benzoic acid (C6H5COOH, Ka = 6.5 × 10-5) in the solution is 0.54 M. What is the concentration of potassium benzoate (KC6H5COO, Kb = 1.5 × 10-10) in this buffer solution?
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
What is the ratio of acetate ion to acetic acid (Ka = 1.76×10–5) in a solution containing these compounds at pH 4.25 ? Write your answer as a decimal and not as a fraction.