3) Yes, the calculated pH of buffer 1 and buffer 2 are same even at different concentrations.
Because, even when the concentrations are different, their relative ratio is the same. As this relative ratio is what affects the pH, they have the same pH
NOTE: The pH of the buffer does not get noticeably affected if the strong acid or strong base added is comparable with the concentration of conjugate base or conjugate acid present in the buffer.
4) pH will not change a lot when a strong acid is added in case of buffer 1A but will change in case of buffer 2A.
In case of buffer 1A when a strong acid is added, H+ in it reacts with the conjugate base present in the buffer whose concentration is comparable in the buffer. So, there will be a very little change in pH
But, the reverse is the case with buffer 2A.
Therefore in buffer 1A, acetic acid equilibrium determines the pH whereas the concentration of strong acid determines the pH in buffer 2A
5) Due to the same reason as in the explanation in NOTE.
pH will not change a lot when a strong base is added in case of buffer 1B but will change in case of buffer 2B.
In case of buffer 1B when a strong base is added, OH- in it reacts with the conjugate acid present in the buffer whose concentration is comparable in the buffer. So, there will be a very little change in pH
But, the reverse is the case with buffer 2A.
Therefore in buffer 1B, acetic acid equilibrium determines the pH whereas the concentration of strong base determines the pH in buffer 2A
PH of Buffered solutions: Acids, If the calculations do not fit into the table, then number the c...
Which of the following are accurate descriptions of buffer solutions? 1. If a solution is buffered, its pH is nearly neutral. II. The mechanism by which buffered solutions resist pH changes is not well understood. III. Addition of strong acid to a buffer shifts the equilibrium such that Ht is consumed. IV. If strong base is added to a buffer, it reacts with the acid component of the mixture. V. Buffers only work well if the one conjugate is present...
Buffers are solutions designed to resist changes in pH from the addition of small amounts of acids or bases. Buffers are comprised of a solution of a weak acid with its conjugate base. When an outside base is added to the buffer, the weak acid in the buffer neutralizes the hydroxide ion of the base, thus retarding its ability to raise the solution's pH. When an outside acid is added to the buffer, the conjugate base of the buffer neutralizes...
Post Lab Activity Acids, Bases, pH, and Buffers 1. Calculate the pH of a 0.08 M NaOH solution. 2. Hydrochloric acid is a strong acid and dissociate almost 100% in aqueous solution. If two drops (0.1 mL) of 1.0 MHCI are added to pure water to make 1.0 L solution. What is the pH of this solution? 3. M. What will be the A dilute solution of hydrochloric acid (HCI) has a concentration of 0.1 pH of this solution? 4....
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...
This is from a Study of Buffer Solutions and pH of Salt Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value larger than the standard value? Procedure: 10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
Calculate the pH expected for the 0.0100 M HCl solution used in part A. I'm so lost please help Intermediate value Final value 1a. Calculate the pH expected for the 0.0100 M HCl solution used in part A. 1b. Calculate the percent error between the expected pH and your measured pH of the 0.0100 M HCI. our To ☺ QUESTION 2 Intermediate value Final value 2a. Calculate the pH of 0.100 M CH3COOH (approximation method). Kg = 1.8 x 10-5...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
help with these chemistry questions 1. Explain what happens to the concentration of H,O' ions in an acetic acid solution when solid sodium acetate is added. 2. Determine the pH and pH of a solution that is 0.5 M NaHSO4 and 0.25 M Na2SO4 3. When sodium nitrite is added to HNO2(aq) a) the equilibrium concentration of HCOOH(aq) decreases. b) the pH of the solution increases. c) the K increases. d) the pH of the solution does not change. e)...
Table 18.2 (continued) 18.20 Solutions Tested pH [H(M) [C,H,O, (M) Percent Dissociation | 0.10 M HCH 0, 2.14 0.010 M HCH 0, 13.09 0.0010 M HC,H,O 284 Question Write the net ionic equation describing the dissociation of acetic acid in aqueous solution. Question Calculate (H) and C.H.O.- for each concentration above, showing a sample cal- culation here Question Write the equilibrium constant expression for acetic acid, and calculate a Kvalue and an apparent percent dissociation for each concentration, showing sample...
Can anyone please help with how to calculate degree of ionization for the first 3 solutions as well as how to calculate the expected pH for solution 4? thank you! Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...