5)Below each titration curve, identify what solution was in the flask at the beginning of thetitration first and what solution was titrated into the flask. Ex: Strong acid - Strong base310Hda20E420141080C1510Acid-Base Titration2030Volume of TitrantAcid-Base Titration2090Volume of Titrant4040A11350C...50(0J1210862HdO141210801010Acid-Base Titration2030Volume of TitrantAcid-Base Titration203020B.4050D50606)Calculate the pH of the resulting solution when 15.00 mL of 0.15 M HNO3 is titrated with20.00 mL of 0.10 M KOH. Include a balanced chemical equation (molecular, ionic, or net ionic) in yourwork. A change table is not required but might be VERY helpful!

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5) titration first and what solution was titrated into the flask. Ex: Strong acid - Strong base 20 مرمت 1 24 12 Below each titration curve, identify what solution was in the flask at the beginning of the 10 D C 15 Acid-Base Titration 10 20 30 Volume of Titrant Acid-Base Titration 20 40 GR C... A 40 50 50 E0 14 12 10 8 6 14 2 12 10 Acid-Base Titration 20 30 Volume of Titrant Acid-Base Titration 40 B. 50 D

5) titration first and what solution was titrated into the flask. Ex: Strong acid - Strong base 20 مرمت 1 24 12 Below each titration curve, identify what solution was in the flask at the beginning of the 10 D C 15 Acid-Base Titration 10 20 30 Volume of Titrant Acid-Base Titration 20 40 GR C... A 40 50 50 E0 14 12 10 8 6 14 2 12 10 Acid-Base Titration 20 30 Volume of Titrant Acid-Base Titration 40 B. 50 D

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 34QRT

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Similar questions

Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Draw the general titration curve for a strong acid titrated by a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What reaction takes place in a strong acidstrong base titration? How do you calculate the pH at the various points along the curve? What is the pH at the equivalence point for a strong acidstrong base titration? Why?
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Compare conductivity titration to pH-metric titration. Do both methods yield the same equivalence point?
2. Below is a titration curve generated by a similar titration to the ones simulated, Vinegar Titration Curve 14.00 13.00 12.00 11.00 10.00 9.00 8.00 * 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 Volume NaOH (mL) We can use this curve to estimate the pka of our weak acid by what is called the "half equivalence point method". The equivalence point is the middle of the steepest part of this graph. Estimate the volume of NaOH added to the titration at that point by using a rule or other straight edge to follow that point down to the x-axis. Divide that volume by 2 (half the equivalence point) and estimate the pH at that volume of NaOH using your straight edge again. pKa = pH at the half equivalence point. What do you estimate the pka to be? 3. The pka of acetic acid is 4.76. Calculate percent error between the true value and your estimated value from question 2.