What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with Ka-35x 1o-8?...
What is the hydronium ion concentration of a 0.210 M hypochlorous acid solution with K = 2.9x10-87 The equation for the dissociation of hypochlorous acid is: HOCl(aq) + H2O(1) = H2O+(aq) + OCH(aq) 0.210 M O 7.8x10-5 M O 7.8*10-4 M O 6.1x10-9 M
what is the hydronium ion concentration [H3O+] and the ph of a 0.5M acetic acid solution with Ka=1.8x10^-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H2O(l) = H3O + (aq) + CH3CO2-(aq)
Question 27 What is the hydronium ion concentration in a 0.5 M ammonia solution? (1 point) 3.0E11 M 3.1E-15 M 3.3E-10 M 3.3E-12 M Question 28 Identify the conjugate acid in the following reaction, HNO3(aq) + H2O() - NO3- (aq) + H3O+ (aq). (1 point) H20 H30+ NO3- None of the above Question 29
Calculate the hydronium ion concentration in an aqueous solution of 4.86x10-2 Mascorbic acid, H,CH06 (aq). [H30*]= M. Submit Answer Retry Entire Group 8 more group attempts remaining Calculate the concentration of HCO3 in an aqueous solution of 0.2440 M carbonic acid, H2CO3(aq). [HCO3]= M. Submit Answer Retry Entire Group 8 more group attempts remaining
What is the hydronium-ion concentration of a 0.140 M oxalic acid, H.C_0.. solution? For oxalic acid, Ka = 5.6 10 and Kay = 5.1 x 10 O 8.4 10 M 3.2 x 10-2M 0 65 % 102 M O 1.1 102 M
A 50 mL sample of 0.150 M hypochlorous acid (one of weak acids) is titrated with a 0.150 M NaOH (one of strong bases) solution. The acid-base equation is as follows: HClO (aq) + OH-(aq) → H2O(l) + ClO-(aq) What is the pH after 25 mL of base is added?
Find the hydronium ion concentration and pH for the following 1. 2. Calculate the hydronium ion concentration and the pH when 80.0 mL of 0.55 MNH, is mixed with 80.0 mL of 0.55 M HCl (K. = 5.6 x 10-10). Concentration M pH- Phenol (CH-OH), commonly called carbolic acid, is a weak organic acid. C, H, OH(aq) + H2O(0) = CH.0 (aq) +H3O+ (aq) K= 1.3 x 10-10 If you dissolve 0.593 g of the acid in enough water to...
A 0.10 M solution of a weak monoprotic acid (HA) has a hydronium-ion concentration of 4.2× 10⁻⁴ M at equilibrium. What is the acid-ionization constant, Ka, for this acid?
1. a)The hydronium ion concentration of an aqueous solution of 0.56 M phenol (a weak acid), C6H5OH, is [H3O+] = ? M b)The hydronium ion concentration of an aqueous solution of 0.558 M pyridine (a weak base with the formula C5H5N) is [H3O+] = ? M. 2. a)The pOH of an aqueous solution of 0.445 M acetylsalicylic acid (aspirin), HC9H7O4, is .? b)The pH of an aqueous solution of 0.517 M aniline (a weak base with the formula C6H5NH2) is ?....
Part A A 0.150 M weak acid solution has a pH of 2.97. Find Ka for the acid. Part B Find the percent ionization of a 0.195 M HC2H3O2 solution. (The value of Ka for HC2H3O2 is 1.8×10−5.) Part C Find the pH of a 0.0191 M solution of hypochlorous acid. (The value of Ka for hypochlorous acid is 2.9×10−8.) Part D Find the pH of a 0.014 M solution of HF. (The value of Ka for HF is 3.5×10−4.) Part...