A 1.00 liter solution contains 0.25 M ammonia and 0.33 M ammonium perchlorate. If 0.170 moles of sodium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of sodium hydroxide.) True A. The number of moles of NH3 will increase. False v B. The number of moles of NH,* will remain the same. True v C. The equilibrium concentration of H,0* will remain the same. False v D. The pH will decrease. True E. The ratio of [NH)/ [NH, will remain the same. An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.

The pH of a sodium acetate-acetic acid buffer is 4.40. Calculate the ratio Note: Reference the K of acids at 25 °C table for additional information. x10 CH₂COO CH₂COOH Be sure your answer has the correct number of significant digits.

Question 18 of 30 Submit A 20.0 mL solution of NaOH is neutralized with 26.3 mL of 0.200 M HBr. What is the concentration of the original NaOH solution? | M 1 4 6. C 7 +/- x 10 0 Tap here or pull up for additional resources 3. LO 00

Each row or the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. dlo initial type (check all that apply) effect of change on pH (check one) solution initial components change O acidic рH higher H,0, HI add Nal A basic pH lower neutral pH the same acidic pH higher B H,0 basic add K Br pH lower neutral pH the same acidic рH higher H,0 basic add KOH pH lower neutral pH the same acidic рH higher H,0, HI D basic add Na OH pH lower neutral pH the same O OO O OO O O O O