Assuming that base (B:) and acid (AH) are mixed in equal concentrations and using pKa values of acid AH 3.5 and pka value of conjugate acid for the base BH 5.5 calculate what percent of BH will appear in this reaction once the equilibrium is reached. Answer is numerical. Round the answer to the nearest whole number. Don't write % symbol in the answer.

Weak Acids and Buffers Write out the simple equilibrium of a weak acid (HA), labeling the conjugate acid and the conjugate base. ● Write out the Henderson-Hasselbalch equation and use this expression to define the meaning of the characteristic pką value.

Determine the Kb for a base by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT > The pH for a 0.0160 M solution of CH:CH.NH: is 8.600. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. CH:CsH&NH:(aq)+ H:O(1) OH-(aq) +CH:CeH&NH;*(aq) Initial (M) |Change (M) Equilibrium (M) 5 RESET 0.0160 8.60 -8.60 0.93 -0.93 2.50 x 109 -2.50 x 109 3.98 x 10 -3.98 х 10° 5.4 -5.4

Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. acid B C Ka M 0 7.28 x 10 pK 1.17 11.3 0 relative strength (Choose one) ✓ (Choose one) ✓ (Choose one) ✓ O *10 X ?

Provide your view on this?  Strong bases have weak conjugate acids with high pKa values, usually > 12.

Solve correctly please.

1. The pKa of HX is 9.34.  Calculate the pH of a 0.418 M solution of HX.  2. A weak monoprotic acid, HA dissociates by 2.416 % and has a pH of 3.61.  Calculate the Ka value for the acid HA.  Record your answer in scientific notation to 3 sig figs.