A volume of 500.0 mL of 0.110 M NaOH is added to 525 mL of 0.250 M weak acid (Ka = 2.53 × 10-'). What is the pH of the resulting buffer? НА(аq) + ОН (aq) Н,О() + А (аq) >
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- 134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO3 is added dropwise to this solution from a burette. Given: Ka (sorbic acid) = 1.7 × 1O^-5 Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above. Suppose that the titration continues. Determine the pH of the solution in the flask at theequivalence pointa.) A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph attached. (i) What is the approximate pKa of the acid? (ii) What specific value from the graph is needed, in addition to the information in part (a) above, to calculate the molar concentration of the NaOH(aq) ? (iii) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated is less than the concentration of its conjugate base.A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3HO-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notation
- Propanoic acid that, along with its sodium salt, can be used to make a buffer that has a pH of 5.25. If you have 512.5 mL of a 0.272 M solution of that acid, how many grams of the corresponding sodium salt do you have to dissolve to obtain the desired pH? For propanoic acid, HC3H5O2, Ka = 1.3 x 10-5. m(salt) = Want solution ASAPBenzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) -> C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10^-5 Calculate the pH of the solution after the following amounts of NaOH have been added… A. 0 mL B. 10 mL C. 85 mLThe weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. a) Sketch the pH vs volume of added base titration curve for this reaction. pH vertically, volume of base horizontally. Label your axes with correct pH and volumes. (Attach more space, if needed) b) what is the pH at the beginning of the titration, Vbase = 0.00 mL ? c) what is the volume of the base needed to reach the equivalence point ? (label the equiv. point) d) what is the pH at the equivalence point?e) what is the pH of the titration when 5.00 mL of base have been added ? f) what is the pH when the volume of base added equals half the volume of the equivalence point? g) what is the pH of the titration when 20.00 mL of base have been added? h) what is the pH of the titration…
- 500.0 mL of 0.1600.160 M NaOH is added to 585585 mL of 0.2500.250 M weak acid (?a=6.71×10−5 MKa=6.71×10−5 M). What is the pH of the resulting buffer? HA(aq)+OH−(aq)⟶H2O(l)+A−(aq) ph=??What is the maximum volume (ml) of 0.195 M Ca(OH)2that can be titrated into 50.0 ml of a buffer comprising0.337 M acetic acid and 0.235 M sodium acetate,before depleting the buffer capacity.Give your answer to 3 significant figures?A buffer system has 3[HA]=[A-]. Given that the pKa is 7.2, what is the pH of the buffer solution at 25°C? Please space stuff out, everything has been written together as a single line so it is difficult for me to figure out what was written
- 16.The titration of an aliquot of 6 mL of acetic acid of commercial use, with NaOH 0.1 , was made by titration, so that to reach the equivalence point 40 ml of NaOH were consumed.Determine the percentage concentration (m/m) of the acetic acid, if its density is 1.05 g/ml. HC2H3O2 acetic acidThe weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. A. What is the pH at the beginning of the titration, Vbase = 0.00 mL? B. What is the pH at the equivalence point? C. What is the pH of the titration when 5.00 mL of base have been added? D. What is the pH when the volume of base added equals half the volume of the equivalence point? E. What is the pH of the titration when 20.00 mL of base have been added? F. What is the pH of the titration when 30.00 mL of base have been added?you are given 1.8 M acetic acid solution (CH3COOH) and solid sodium acetate trihydrate (NaOOCCH3 X 3 H2O) the two buffer solutions are identical. if 5.00 mL of a 1.0 M NaOH solution is added to one of the buffers what would be the resulting pH after addition?