propanic acid, a food additive listed by its E number E280, has a pKa value of...
An organic acid has pKa = 8.95. What is its Ka value? Where does the acid fit in Table 16.2?Table 16.2 Ionization Constants for Some Acids and Their Conjugate Bases at 25°C?
A certain organic acid has a Ka of 5.01 × 10−4. What is its pKa?
A certain inorganic acid has a pKa of 5.8. what is its Ka?
enter answer in scientific notation.
2 attempts left Check my work A certain inorganic acid has a pK, of 5.8. What is its K,? Enter your answer in scientific notation. Be sure to round your answer to the correct number of significant figures. K - T X 10 (select) References eBook & Resources
A certain acid has pKa = (7.997x10^0). What is the acid's Ka? (Ka, Kb, pKa, and pKb are unitless quantities.)
7. The p-fluorobenzoic acid (C6FH5CO2H) has a pka = 4.14 a) Compute the Ka value for this acid. (4 points) b) Compute the Ko value for the conjugate base of this acid above and write out the equilibrium of the conjugate base. (6 points) c) Calculate the pH of a 0.0572 Molar sodium fluorobenzoate ( Na C6FH5CO2 )solution. Use the equilibrium in b to start this problem and the Kb from above. (8 points)
Please Explain: 7) a. Why does an acid and its conjugate base have the same pKa and Ka values? b. Why does a base and its conjugate acid have the same pKa and Ka values? Thank You! <3
Base/Acid Ratios in Buffers Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, pKa=?logKa The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH=pKa+log[base][acid] Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. Part A Acetic acid has a Ka of 1.8
Boric acid has a Ka of 5.8 × 10-10. What is the pKa? Assume boric acid is H3BO3 and is monoprotic.
QUESTION 3 Given the following pka values, which is the strongest acid of those listed in the answers? HClO2 (pka = 2.00) CCI3COOH (pKa = 0.52) HIO3(pka = 0.77) HBrO2 (pka = 4.69) HN3 (pka = 4.72) O A. CClgCOOH B. HBrO2 C.HIO3 D.HCIO2 E. HN3
A 50 mL sample of 0.20 M propionic acid buffer (pKa 4.87 according to Google) has an initial pH of 4.77. After an unknown amount of 0.25 M HCl is added to the buffer, its pH has been lowered to 4.47. Using the Henderson-Hasselbalch equation, determine what volume of HCl was added to the buffer to cause the pH change, as well as the mass of Pr- necessary to return the buffer to its original pH.