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- Only typed explanation otherwise leave it The acid ionization constants of sulfurous acid (H2SO3) are Ka1 = 1.7 × 10−2 and Ka2 = 6.4 × 10−8 at 25.0 °C. Calculate the molar concentration of hydrogen sulfite ion of a 0.163 M aqueous solution of sulfurous acid. ANS: 0.045 Can you please show me how you get this answer!What is the pH of 500ml solution conating 0.125 M fornic acid and 0.140 M sodium formate? Include chemical equation What would the pH be if 1mL of 0.5 HBr was added to solution? pka=3.744Which of the following will not act as a Bronsted base in water at 298 K, and not participate in hydrolysis? [Select all that apply] Group of answer choices Cl− F− OH− NO3− I− Br− ClO3− ClO4− NH3 ClO− PreviousNext
- Chemistry Which of the following species is not amphiprotic? (circle all that apply) H2O, HSO4-, Ca(OH)2, C2H3O2H, H2S, CH3NH2 Please explain this question.Show all work. Please 1) Write equations that show H2PO4− acting both as an acid and as a base. 2) Calculate the pH and the pOH of each of the following solutions at 25 °C for which the substances ionize completely: (a) 0.200 M HCl (b) 0.0143 M NaOH (c) 3.0 M HNO3 (d) 0.0031 M Ca(OH)2 3)Propionic acid, C2H5CO2H (Ka = 1.34 × 10−5), is used in the manufacture of calcium propionate, a food preservative. What is the hydronium ion concentration in a 0.698-M solution of C2H5CO2H?1) LiF has a pKsp of 2.77. HF has a pKa of 3.17. LiF is dissolved at 0.250 F after addition of strong acid. What is the pH of the 0.250 F LiF solution? Answer: 1.62 2) For the problem above, how many moles of strong acid are added to form 1.000 L of solution? Answer: ? Please solve the second question, not the first question.
- How would I answer these questions? I have gotten an answer but I want to confirm im on the right way. Here are my questions: 1. What is the concentration of the OH- ion in 0.03 M HCl? 2. What molarity of butanoic acid (pka) = (4.82) would have a pH of 3.0?4. Calculate the pH of a 0.340 M NaO₂CCO₂H solution. pK₁ = 1.250 and pK2 = 4.266. Please type answer not write by hendProblem Solving. Solve the following problems, use GRESA format in answering A 0.0001 molar basic solution is 1.50 % ionized. What is the pH of the solution if its Kb= 1.25 × 10^−6?
- (please see pictures attached for reference. I tried my best) 27. Dissolved dioxygen in water samples can be determined by the following equations:2MnSO4(aq) + 4NaOH(aq) + O2(g) --> 2MnO2(s) + 2Na2SO4(aq) + 2H2O(l)2MnO2(s) + 2H2SO4(aq) + 2NaI(aq) -->MnSO4(aq) + I2(aq) + Na2SO4(aq) + 2H2O(l)I2(aq) + 2Na2S2O3(aq) --> Na2S4O6(aq) + 2NaI(aq)A water sample from the local river was treated according to the first two equations above. Exactly 200.00 mL ofthis treated water required 8.32 mL of 0.0250 M Na2S2O3 to titrate to the endpoint. Calculate the concentration ofdissolved oxygen in the water sample.A) 1.04 x 10-3MB) 2.08 x 10-4MC) 5.20 x 10-4MD) 8.67 x 10-7ME) 4.33 x 10-7M 28) How many neutrons are needed to initiate the fission reaction shown? 23592 U + ? 10 n --> 13956 Ba +9436 Kr+ 310n a) 0 b) 1 c) 2 d) 3 e) 5 20. Consider the substances H2O, KI, H2S, CH4. Which answer has the substances arranged in order ofDECREASING boiling point?a) KI > H2O > CH4 > H2S b) KI…The pH of 8.35 is wrong, but I'm not sure how to get the right answer36. Lactic acid is a weak acid with the formula HC3H5O3, the Ka for lactic acid is 1.38 x 10-4 In aqueous solution, lactic acid partially dissociates according to the following reaction: HC3H5O3 + H2O ⇔ C3H5O3- + H3O+ Calculate the pH of the lactic acid solution described below: Volume: 250 mL Concentration: 0.2931 M Since this is a weak acid, you can assume the amount of acid dissociated is << 5% of the total amount of acid present.