QUESTION 4 The Ka of HCHO2 is Ka=1.8 x 10-4. What is the value of Kb...
QUESTION 1 The Ka for HCHO2 is 1.77 x 10-4 What is the value of the equilibrium constant for the reaction: H+ (aq) + CHO2 (aq) HCHO2 (aq)? 0 1.77 x 10-4 O 5.65 x 103 0 1,00 x 10-14 O 5.65 x 10-11
Find the pH of a 0.011 M solution of HCHO2. (The value of Ka for HCHO2 is 1.8×10?4.)
Calculate the pH of a 0.0107 M sodium formate solution. Ka (HCHO2) = 1.8 × 10−4. Report your answer to TWO places past the decimal.
Given that Ka for HCOOH is 1.8 � 10-4 at 25 �C, what is the value of Kb for COOH� at 25 �C? Kb=5.56 x10^-11 Given that Kb for CH3CH2NH2 is 1.7 � 10-9 at 25 �C, what is the value of Ka for CH3CH2NH3 at 25 �C? Ka=
What is the hydronium concentration of a 0.0895 M formic acid, HCHO2, solution. Ka (HCHO2) = 1.8 x 10-4
PartA Given that at 25.0C Ka for HCN is 4.9 x 10-10 and Kb for NH is 1.8 x 10 calculate Kb for CN and Ka for NH4+. Enter the Kb value for CN followed by the Ka value for NH4,separated by a comma, using two significant figures. View Available Hint(s) Submit
The Ka for ch3co2h is 1.8 x10^-5 and the Ka for ch2chco2h is 1.4x10^-3. what is the Kb of the weaker of their two respective conjugate bases? a. 2.1 x10^-8 b. 7.1 x10^2 c. 6.7 x 10^-10 d. 6.7 x 10^4 e. 7.1 x 10^-12
Determine the pH of each of the following solutions. 0.19 M KCHO2 (Ka for HCHO2 is 1.8×10−4) 0.15 M CH3NH3I (Kb for CH3NH2 is 4.4×10−4) 0.18 M KI
Determine the pH for each of the following solutions: 0.22 M KCHO2 (Ka for HCHO2 is 1.8×10−4) 0.18 M CH3NH3I (Kb for CH3NH2 is 4.4×10−4) 0.25 M KI
Given that Ka for HCN is 6.2*10^-10 at 25°c, what is the value of Kb for CN- at 25°c? Given that Kb for NH3 is 1.8*10^-5 at 25°c, what is the value of Ka for NH4+ at 25°c?