omework ubmitted Aug 8 at 11:15pm 1/1 pts Question 13 The [OH ] and the pH of 0.035 M KOH at 25 °C are, respectively, 0.035 M and -1.46 0.035 M and +1.46 O 2.9 x 10 13M and -12.5 0.035 M and +12.5
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- The pH of an aqueous solution of 0.0655 M ammonium bromide, NH4 Br(aq), is (Assume that K₁ (NH3) = 1.80 x 10-5.) This solution is Submit Answer Retry Entire Group 1 more group attempt remainingWhich of the following equations represents the acid equilibrium associated with Ka, for H3PO3? A) HPO,²- (aq) + H20 (1) = PO;3- (aq) + H;0* (aq) B) H;PO, (aq) + H,0 (1) = H,PO;¯ (aq) + H,0* (aq) = H¿PO;- C) H,PO,- (aq) + H,0 (1) = H,PO3 (aд) + ОН- (аq) D) H,РO;- (аq) + H,0 () (aq) + H30* (aq) HPO,2-n aqueous splution contaiOS 0.100 M NADHH at 25.0°C. the PH of the gokution is
- What is the pH of a grapefruit that contains 0.007 M citric acid solution (CsH2O-)? CH;O;(aq) + H;O(2) = CH;0, (aq) + H3Oʻ(aq) K, = 7.5 x 104 Round your answer to 2 decimal places.What is the pH of a grapefruit that contains 0.007 M citric acid solution (C;HgO;)? CH3O;(aq) + H2O(2) = CGH;0, (aq) - H30ʻ(aq) K, = 7.5 x 104 2.71 3.62 5.35 4.54Calculate the pH and the pOH of these solutions: (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH = pOH =
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- 6. (i) Define pH in words. The strong acid HClag has a pH value of 1, use the following equation for a strong acid: HClaa Hog + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] Clea (ii) Use the above expression to deduce the pH of HCl (ag) given the concentration of the acid to be 4.5 mol/dm³ pH =A 0.15-M aqueous solution of a weak acid HA has a pH of 5.35 at 25oC. What is the Ka of the acid? (A) 4.5 x 10–6 (B) 2.2 x 10–9 (C) 1.3 x 10–10 (D) 2.0 x 10–11Determine the pH of each of the following solutions.(a) 0.684 M hypochlorous acid (weak acid with Ka = 3e-08).(b) 0.399 M hydrogen peroxide (weak acid with Ka = 2.4e-12).(c) 0.751 M pyridine (weak base with Kb = 1.7e-09).