In acid base titration, generally there is a titrant ( an unknown which concentration to be calculated ) and a titrand (a solution with known concentration) is taken.
Generally our titrants are acids, which pH are to be calculated, taken in a flask or beaker. And the titrand is a strong base which is taken in a burrette and added to the acid in flask dropwise untill it reaches the equivalance point.
Now in the question, our titrand is a strong base NaOH.
Again equivalance point is that point where all the NaOH added have been completely used in neutralizing the acid present. Thus at this point, all the acids are converted to its salt of conjugate base. Thus will form a buffer
a-
Here both the given acids C6H5-CO2H and ClCH2CH2CO2H are weak acids. Now pKa for C6H5-CO2H = 4.20 and pKa for ClCH2CH2CO2H = 2.87
We know lesser the pKa, stronger is the acid. Thus between these pair, ClCH2CH2CO2H is a stronger acid than C6H5-CO2H.
The pH of a buffer is calculated by Henderson Hasselbalch equation-
pH = pKa + log [salt]/[acid]
If we consider for a particular acid, then its pKa value is always same. That means the change in pH depends upon the change in concentration of salt and acid. Higher the [salt] and lower the [acid] will produce a higher log [salt]/[acid] value. Thus a higher change in pH value is observed.
Now generally weaker acids corresponds to greater changes when strong bases are added. Thus they will provide a greater change in pH.
On this basis, C6H5-CO2H will produce greater change in pH on addition of NaOH
2- Similarly Here both the given acids HF and HCO2H are weak acids. Now pKa for HF = 3.1 and pKa for HCO2H = 3.74
That means HCO2H is the weak acid in the pair. Hence HCO2H will produce greater change in pH on addition of NaOH
6. Identify the titrant in each pair that would provide a greater pH change about the...
7. Identify the titrant in each pair that wou ld provide a greater pH change about the equivalence point in the titration of a 0.100 M HCI solution. Explain your reasoning for your choice for each pair. a) 0.10 M dimethylamine ((CH3)2NH) or 0.10 M ethylamine (CH3CH2NH2) (2 pts) b) 0.10 M carbonate anion (CO32) or 0.10 M cyanide anion (CN) (2 pts)
What is the pH at the equivalence point in the titration of 50.0 mL of 0.100 M hydrofluoric acid, HF, (Ka = 7.2 x 10-4) with 0.100 M NaOH?
24A) 40mL of 0.2 M formic acid is titrated with a strong base (NaOH= 0.5 M). Determine the pH before any base has been added. Please show steps and please explain why the answer is what it is. 24B) The 40mL 0.2 M formic acid is titrated with a 6.0mL of strong base. Here NaOH can be treated as a conjugate base and formic acid is the acid. please show steps and explain! Us (24-25, Acid/base, aqueous equilibrium) 24A) (4...
3. The following titrations are all at their equivalence points. Rank the solutions from highest to lowest pH at the equivalence point and explain your reasoning. a. 20.00 mL of 0.10 M NaOH + 10.00 mL of 0.20 M acetic acid b. 20.00 mL of 0.10 M NaOH + 10.00 mL of 0.20 M chloroacetic acid c. 10.00 mL of 0.20 M NaOH + 20.00 mL of 0.10 M HCI
(3) 30.00 mL of 0.085 M Hydrofluoric acid (HF) is titrated with 0.10 M NaOH. What is the pH of the acid solution before any base is added? (Ans: pH = 2.11) What is the pH of the titration mixture at half the equivalence point? (Ans: pH = 3.35) What is the pH of the titration mixture at the equivalence point? (Ans: pH = 7.92) What is the pH of the mixture after 40.00 mL of base are added? (Ans:...
Learning Goal: To learn about titration types and how to calculate pH at different points of titration. In an acid-base titration, a titrant (solution of a base or acid) is added slowly to an analyte (solution of an acid or base). The titration is often monitored using a pH meter. A plot of pH as a function of the volume of titrant added is called a pH titration curve. Prior to the titration, the pH is determined by the concentration...
1. A buffer is 0.100 M in HF and 0.100 M in NaF. When a small amount of nitric acid is added the pH only slightly drops. Write the chemical equation that shows the added nitric acid being neutralized by this buffer. 2. What is the pH of a buffer that is 0.120 M formic acid (HCHO2) and 0.080 M in potassium formate (KCHO2)? The Ka of formic acid is 1.8 x 10^ -4 . 3. The curve shows the...
2. Weak Acid versus Strong Base Derive a titration curve for the titration of 50.0 mL of 0.100 M formic acid, HCHO2 (Ka 1.80 x 104) with 0.100 M N2OH. Calculate the pH for the following volumes of NaOH (0 mL, 10 mL, 25 mL, 40 mL, 50 mL, 55 mL, 60 mL). Volume of N2OH, in milliters pH (a) (b) (c) (d) (e) (f) (g) 0 10 25 40 50 55 60 pH at the equivalence point Specify your...
Problem Set 16 CHEM 1252 November 13, 2019 2. Consider the titration of 60.0 mL of 0.024 M NaOH with 0.036 M HCI. write the net lonication for the Histor i cading physical states. What is the eldrons p between this reaction and an antalysis reaction Given this retro what is the equilibrium constant for the titration reaction and why can we safely assume that it woes completion"7 Why should you expect the pH to equal 7.00 at the equivalence...
PRE-LAB for pH titration of a Strong Acid with Base This is due before the lab begins, Name 1. Calculate the pH of the following solutions: (a) 1 M NaCl Does not dissociate in water to produce either hydrogen or nyot thus it is a neutral Sall, so 7. (b) 1 M HOAc (Ka - 1.8 x 10-5) duce either hydrogen or hyd xde ion, (c) 1 M NHOH (Kb = 1.8 x 10-5) (d) 0.1 M NaOAC (e) 0.1...