An initial solution is made by combing 13 mL of 0.8 M chloroacetic acid with 20 mL of a NaCH2ClCOO solution. (Ka= 1.4x10-3)
a) The pH of the resulting solution was measured to be 2.92. What is the concentration of the NaCH2ClCOO solution?
b) The solution from part a) is then titrated with 5 mL of 0.8 M NaOH. What is the pH of the resulting solution?
c) If the solution is then titrated to its equivalence point, how much more NaOH solution must be used?
d)What is the pH of the solution at the equivalence point?
An initial solution is made by combing 13 mL of 0.8 M chloroacetic acid with 20...
Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium hydroxide. The volume of 27.40 mL of NaOH(aq) was needed to reach the equivalence point. Calculate: a) The concentration of the chloroacetic acid solution before the titration b) the pH of the chloroacetic acid solution before titration c) the pH of the solution at half equivalence point d) the pH of the solution at the equivalence point e) the pH of the solution when...
A 25.0 mL sample of 0.150 M chloroacetic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The of chloroacetic acid is 1.4 ×10-3.
What is the pH of the solution when 100 mL of 0.8 M formic acid (Ka= 1.8x10-4) is titrated with 50 mL of 1.2 M NaOH? 1.80 grams of an unknown monoprotic acid (HA) required 48.62 mL of a 0.25 M NaOH solution to reach the equivalence point. Calculate the molar mass of the acid. Need help understanding please show work. Thank you in advance.
Please show steps and thought process.
Suppose you have a 50.00ml of 0.0100 M chloroacetic acid solution, HC_2H_2O_2CI. K_a=1.40 Times 10^-3. What is the initial pH for this solution? What is the equivalence point pH if the chloroacetic acid was titrated with 0.0100M NaOH?
What is the pH of a solution of 40.0 mL of 0.100 M acetic acid (Ka = 1.8 x 10-5) after 50.0 mL of 0.100 M NaOH has been added? Calculate the concentration of dissolved Ba2+ ions when BaSO4 is added to water at 25°C. Кsp? = 1.10 x 10-10 A particular saturated solution of silver chromate (Ag2CrO4), has [Ag+] = 5.0 x 10 Mand (CrO4) = 4.4 x 10M. What is value Ksp for silver chromate? As a result...
3.)A certain weak acid, HA, with a Ka value of 5.61×10?6, is titrated with NaOH. Part A A solution is made by titrating 7.00 mmol (millimoles) of HA and 1.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. Part B More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 35.0 mL ?...
A 50.0 mL sample of 0.25 M formic acid (HCOOH) aqueous solution is titrated with 0.125 M NaOH solution. Ka of HCOOH = 1.7 x 10−4. a. Calculate the pH of the solution after 50 mL of NaOH solution has been added. b. How many mL of 0.125 M NaOH need to be added to the sample to reach the equivalence point? What is the pH at the equivalence point?
2)250.0 mL of a 0.375 M solution of lactic acid (HC:H:03) is titrated with a solution of 0.75 M NaOH. The K, for lactic acid is 1.38 x 104. (22 pts total) a) what is the pH before addition of NaOH? (Hint: what is the relevant equilibrium?) (4 pts) b) what is the total number of moles of acid? (2 pts) c) what volume of the NaOH solution is required to reach the equivalence point? (2 pts) d) what is...
A solution of 100. ml of .500 M Acetic Acid is titrated with .500 M sodium hydroxide. The Ka of acetic acid is 1.8*10^-5. Find the pH values at the given stages: a) before the addition of any NaOH. B) After 25.0 mL of NaOH added. C) At the equivalence point.
A 25.0 mL sample of 0.150 M formic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of formic acid is 1.8 ⋅ 10-4.