Question 39 1 pts A weak acid (HA) reacts with a weak base (B) to form the conjugate base of the acid (A) and the conjugate acid of the base (B-H the pKa of HA was 4.8 and the pKa of BH* (i.e., the p...
A weak acid (HA) reacts with a weak base (B) to form the conjugate base of the acid (A-) and the conjugate acid of the base (B-H+). If the pKa of HA was 4.7 and the pKa of BH+ (i.e., the pKabH of B) was 9.4, what would be the value of the equilibrium constant for the above reaction to the nearest ones? Obviously, by expressing the answer to the nearest ones, we are using too many figures than is...
Consider the reaction between a weak acid (HA) and a weak base (B). If the pKa of HA was 4.6 and the pKa of BH was 10.1, what would be the value of the equilibrium constant to the nearest ones? Hint: Once you write the expression for Keq, you should recognize terms that you can "swap out" with equivalent terms from the Henderson-Hasselbalch equation; this should greatly simplify the math.
For the weak base B, pKb = 4.83. Give the value of pKa for the conjugate acid BH+. At what pH does [B]=[BH+]? What is the ratio [B]/[BH+] at pH=7.05? What is the ratio [B]/[BH+] at pH=12.23?
Question 1 (2 points) The relationship between a weak acid and its conjugate base at the 1/2 neutralization point is: the weak acid's concentration is greater than the conjugate base concentration. the weak acid's concentration is less than the conjugate base's concentration the weak acid's concentration is 1/2 the concentration of the conjugate base's concentration the weak acid and conjugate base have the same concentration. Question 2 (3 points) ✓ Saved The pka of acid is 4.8. Determine the acid's...
1. Calculation of pH. A weak acid HA (pKa = 4.85) reacted with strong base NaOH The reaction is HA + NAOH H20 + NaA. There are 100 mL 0.100 M HA solution, and the concentration of Na OH is 0.100 M. 0 moles a. What is the pH when 0.00 mL of NaOH is added to the 100 mL HA solution? 2 x1 les b. What is the pH when 20.0 mL of NaOH is added to the 100...
H aq H g anode An electrochemical cell consists of a H aq 1 .00 M H g) cat ode connected to a which e H concentration a ofa u er cons nu of a weak acid HA(0.116 M), mixed with its conjugate base, A (0.143 M). The measured cell voltage is E°ell 0.163 V at 25 °C, with PH2-1.00 atm at both electrodes. Calculate the pH in the buffer solution and the K of the weak acid. Ka H...
1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...