2. Dr. Dahm has prepared 250 mL of a acetate buffer which contains 0.1 mol of acetic acid (CH₂COOH) and 0.15 moles of acetate (CH₂COO). Determine the initial pH. If he then adds 0.025 moles of H* calculate the new pH. Ka = 1.8 × 10'³ CH₂COOH(aq) + H₂O CH₂COO (aq) + H₂O*(aq) 3. Dr. Dahm makes a second acetate buffer exactly the same way as in #2, but he then adds 15 mL of 0.50 M NaOH calculate the new pH.

Predict the effect of adding HCL aqueous to the equilibrium reaction 

A buffer solution is made that is 0.485 M in HNO2 and 0.485 M in NaNO2 . If  Ka for HNO2 is 4.50 x 10^-4 , what is the pH of the buffer solution? pH =  Write the net ionic equation for the reaction that occurs when 0.137 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)   +       +

Formic acid, HCOOH, is the simplest of the carboxylic acids and occurs naturally, most notably in some ants.  If the formate (HCOO–) concentration is 0.100 M, determine the formic acid (HCOOH) concentration required to buffer a solution at pH = 3.35   HCOOH(aq) ↔ HCOO–(aq) + H+(aq)        Ka = 1.80 × 10-4   i) Calculate the pKa of the acid and provide your final answer with 3 decimal places ii) Write the main equation that you will use to help you calculate the formic acid concentration iii) Calculate the formic acid concentration required to buffer the solution at pH = 3.35 and provide your final answer with 3 decimal places

G.137.

An analytical chemist is titrating 102.2 mL of a 0.5200 M solution of nitrous acid (HNO,) with a 0.5400 M solution of KOH. The p K of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 21.31 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. db pH = Explanation Check © 2021 McGraw Hi Education. All Rights Reserved. Terms of Use Pivacy Accessibitity 5:12 PM P Type here to search 5/8/2021 prt sc delete home end 144 14 4O 144 num lock %23 3. 96 backspace 4. 8. 7. Y. home

A chemistry graduate student is given 450. mL of a 1.00M chlorous acid (HClO₂) solution. Chlorous acid is a weak acid -2 with K = 1.1 × 10 . What mass of NaClO₂ should the student dissolve in the HClO2 solution to turn it into a buffer with a pH = 1.52? You may assume that the volume of the solution doesn't change when the NaClO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. [] x10 X

Titrations are acid-base reactions in which the amount of acid and base in solution are known quite precisely. The specific case where the acid and base have been added in equivalent molar amounts, is called the equivalence point. At this point, mol acid = mol base %3D At all other points in a titration, either the base is the limiting reactant (and there is excess acid) or the acid is the limiting reactant (and there is excess base). So, except at the equivalence point, titration problems are limiting reactant problems, which means we can do them- a lot of them! One additional point: when there is left over strong acid (acid in excess), 100% of that excess acid is ionized to become H* ions: [strong acid] = [H*] and pH = -log[H"] Something similar happens for strong bases. 1. Calculate the pH of the solution after the following amounts of 0.250 M NaOH have been added to 50.0 mL of 0.200 M HCI. Show all your work for each calculation (including the volumes for which the pH is given).…

A volume of 500.0 mL of 0.160 M NaOH is added to 525 mL of 0.250 M weak acid (K₁ = 3.24 × 10-5). What is the pH of the resulting buffer? pH = HA(aq) + OH¯(aq) H,O(l) + A(aq)

A 40.ml solution of 0.100 M sodium hypochlorite is titrated with a 0.100 M HCl solution. Ka (HClO) =3.0 x 10 ^-8. What is the pH of the equivalence point?