1) if concentration of weak acid is increased that means more amount of NaOH now will be required to reach the half equivalence point because acid now becomes more concentrated.
2) If the acid has larger Ka that means higher dissociation constant then H+ will be given out easily and hence volume required to reach half equivalence point will be less and half equivalence point will come early.
3) if NaOH used is highly concentrated then also less NaOH will be required for the titration and half equivalence point will come at EARLY.
When an unknown weak acid is titrated with NaOH, how would your half-equivalence and volume of...
How would the pH for a weak acid at the half-equivalence point and volume of NaOH used as the titrant to reach the equivalence point, change if the i) NaOH concentration was increased ii) Acid concentration was increased
When a weak acid is titrated with a strong base, if the pH at the half-equivalence point is 6.04, what is the Ka of the acid?
It's a weak acid strong base titration Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
5. The Ka and Molar Mass of a Monoprotic Weak Acid a. Suppose that–unknown to you–the primary standard KHP (potassium hydrogen phthalate, KHC8H4O4) had a potassium iodide impurity of approximately one percent by mass. How would this have influenced the calculated molarity of your sodium hydroxide solution? Would your calculated value be too low, too high, or unchanged? Explain your answer. b. Sketch a typical titration curve for a monoprotic weak acid titrated with a strong base. Label the axes...
Weak Acid Titration When a 14.0 mL sample of a monoprotic weak acid is titrated with 0.10 M NaOH, it generates the titration curve shown below. Weak Acid titrated with 0.10 M NaOH pH Volume of 0.10 M NaOH a) What is the molar concentration of the original sample of weak acid? х М b) What is the ka for this weak acid?
1) A solution of a weak monoprotic acid of unknown concentration was titrated with 0.23 M NaOH. If a 100.-mL sample of the acid solution required exactly 10. mL of the NaOH solution to reach the equivalence point, what was the original concentration of the weak acid? 2) During the titration on problem (2B), after 5.0 mL of NaOH addition, the pH = 3.68. What is the Ka of the weak acid? please show steps i have an exam tomorrow
When 30.0 mL of an unknown acid was titrated with 0.323 M NaOH, 33.1 mL of the base was required to reach the equivalence point. What was the concentration of the acid? Please include units in your answer
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyze has reacted to form its conjugate, and the other half still remains unreacted. If 0.4400.440 moles of a monoprotic weak acid (?a=7.2×10−5)(Ka=7.2×10−5) is titrated with NaOH,NaOH, what is the pH of the solution at the half‑equivalence point? pH=pH= 2) A volume of 500.0 mL500.0 mL of 0.120 M0.120 M NaOHNaOH is added to 565 mL565 mL of 0.250 M0.250 M weak acid...
Question 3 (20pts): 20 mL of an unknown weak acid is titrated using 0.02 M NaOH. pH is monitored with a pH-meter and the data below collected (see back of this sheet). A) Create a plot of this titration using the data below. Label the approximate position of the equivalence point on the plot. B) Create a Gran plot using this data. Include the equation of the line that you fit to the data as well as the R2 value....
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water and titrated against 0.1555 M NaOH, requiring 48.11 mL to of NaOH to reach the end-point. During the titration reaction, the pH of the solution is 3.77 when half of the HA is neutralized and the equivalence-point pH is 8.33. (a) State two ways to standardize the NaOH used in the titration. (b) Suggest and explain an indicator that can be used in the...