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- What is the percent ionization of 7.5x10-2 M HCN? Ka = 4.0 x 10-10 for HCN. ** Need asap pls. Thanks.ITTL/ What is the pH of 92.9 mL of a solution which is 0.29 M in NaCN and 0.61 M in HCN? For HCN use K₂ = 4.9x10-10. Your Answer:What is the pH of a 1.000 L solution of 0.100 M HA after the addition of 1.000 L of 0.075 M NaOH? The K₂ of HA is 6.78 * 10 ^ - 8 . Record your answer to two decimal places.
- The propionate ion, CH3CH2COO–, reacts with water as a weak base: CH3CH2COO–, (aq) + H2O(l) ⇄ CH3CH2COOH(aq) + OH–(aq), with K = 7.4 x 10-10 at 25°C. If sodium propionate were dissolved in water to make a 0.60 M solution, what would be the resulting concentration of OH–? (no scientific notation)Helppp nowwowoow please Equation #H+MA.VA=MB.VB #OH- What is the concentration of an unknown Mg(OH) 2 solution if it took an average of 15.4mL of 0.100M solution to neutralize 10.OmL of the Mg(OH) 2 solution ? What is the concentration of an unknown LiOH solution if it took an average of of 0.100M HNO3 solution to neutralize 20.0ml of the solution?I only need help with problem 4 please. 3. The concentration of carbonic acid, H2CO3, in a typical carbonated drink is approximately 7.0 x 10-2 M. Carbonic acid is a diprotic weak acid with the following pKa values for the 1st and 2nd ionizations: H2CO3 + H2O <===> H3O+ + HCO3- pKa = 6.3 HCO3- + H2O <===> H3O+ + CO32- pKa = 10.3 From highest concentration to lowest concentration, what are the molecular and ionic species present in an aqueous solution of 7.0 x 10-2 M H2CO3 (note: you do not have to calculate the concentrations, just rank them in order of highest to lowest). 4. What is [H3O+] and the pH of a solution of H2CO3 with [H2CO3]Total = 4.5 x 10-4 M? (Use the pKa value for H2CO3 given in Problem 3.) Hint: This is not a buffer.
- What is the pOH of a solution of 0.125 M CH3NH2 and 0.130 M CH3NH3Cl? How would you find a Ka value? Calculate [OH-], [H+], and pH for practiceLactic acid, HC3H5O3, is a monoprotic acid that dissociates in aqueous solution. If a solution containing 0.50 M lactic acid is 1.66 percent dissociated to ionic form, calculate the value of Ka for lactic acid. Include answer to 3 significant figuresWhat is pOH of a solution consisting of 1.05 M NH3 and 0.98 M NH4NO3? Ka of NH4 + is 5.8 x 10-10 Group of answer choices 9.07 4.73 4.93 9.27
- Find the percent ionization (?α) of a 3.0 M HNO2 solution. (Ka for HNO2 is 4.6 × 10-4) A) 1.2% B) 2.1 % C) 2.7% D) 3.5 % Group of answer choices A B C DKb for NH3 is 1.8 × 10-5. What is the pOH of a 0.20 M aqueous solution of NH4Cl at 25.0 °C? A) 2.72 B) 11.28 C) 9.02 D) 4.98 E) 11.234. Saccharin, C 1 H 4 NSO 3 H a weak acid (K a =2.1*10^ -2 ) . If 0.250 L of diet cola with a buffered pH of 5.48 was prepared from 2.00 * 10 ^ - 3 * g sodium saccharide, Na(C 7 H 4 NSO 3 ) what are the final concentrations of saccharin and sodium saccharide in the solution? Express your answer in molarity as scientific notation using two significant digits (hint: Henderson-Hasselbach). C 7 H 4 NSO 3 H (aq) +H 2 O (l) rightleftharpoons H 3 O^ + (aq)+C 7 H 4 NSO 3 (