Why can you interchangeably use HB+/B and HA/A- in acid-base equations?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Why can you interchangeably use HB+/B and HA/A- in acid-base equations?
use a diagram to explain why Ha appears more downfield than Hb
or Hc in the 1H NMR.
Acetophenone
H: 87.94 ppm Hb: 87.40 ppm H.: 87.40 ppm
For many weak acid or weak base calculations, you can use a simplifying assumption to avoid solving quadratic equations.
$$ K_{\mathrm{a}}=\frac{x^{2}}{[\mathrm{HA}]-x} \approx \frac{x^{2}}{[\mathrm{HA}]} $$
Classify these situations by whether the assumption is valid or the quadratic formula is required.
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 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...
Consider the Ka values for the following acids: Acid Ka HA 3.77E-5 HB 4.65E-6 HC 6.60E-6 HD 2.84E-4 HE 1.45E-5 Write the formula for the acid which has the STRONGEST conjugate base. What is the corresponding Kb value for the strongest acid from the table above?
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.
10. Which is a stronger acid: A) HA, K. - 4.4x10-10 B) HB, K, -2.6x10* 11. Identify the conjugate acid of CO 2- in the reaction C0,2- + H2POCHCO,- + HPO42- A) H.CO B) HCO3- C) H20 D) HPO, E) H2PO4 12. Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 x 10 M A) 2.34 B) 3.47 C) 6.01 D) 7.99 E) 10.53
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 Ka values for the following acids: Acid ka HA 4.40E-6 HB 7.01E-6 HC 1.24E-5 HD 3.38E-5 HE 1.25E-5 Write the formula for the acid which has the STRONGEST conjugate base. Submit Answer Tries 0/98 What is the corresponding Kb value for the strongest acid from the table above? Submit Answer Tries 0/98
Use the Acid-Base Table to write net equations and to determine the equilibrium constants for the Bronsted acid-base reactions that occur when aqueous solutions of the following are mixed. See the instructions for writing chemical equations given above. Reactants Acid(1) + Base(2) = Base(1) + Acid(2) K a) HClO4 and KF b) HIO3 and NH3 c) HCN + KClO Click here to preview your answer.
19.2A The molecular scene below shows a sample of an HB/B buffer. (HB is blue and yellow, and B is yellow, other ions and water are not shown.) MODEL Od slo Hotellbarer a) Would you add a small amount of concentrated strong acid or strong base to increase the buffer capacity? Why? b) Assuming no volume change, draw a scene that represents the buffer with the highest possible capacity after the addition in part (a).