Strong Bases/Acids vs. Weak Bases/Acids The 4 Titration Curves Combinations NaOH + HCI Strong Base Strong Acid Strong Base+ Weak Acid HOOD HO+ HOEN Weak Base Strong Acid IOH + HO'HN NH.OH + CH.COOH Weak Base Weak Acid 4. Explain why the titrations which began with CH3COOH started from a higher pH value compared to those which began with HCI. 5. What was the purpose of adding the indicator to each titration? 6. Two titrations ended with the pH well above 10 the other two titrations ended with the pH below 10. Explain why this occurred.

Strong Bases/Acids vs. Weak Bases/Acids The 4 Titration Curves Combinations NaOH + HCI Strong Base Strong Acid Strong Base+ Weak Acid HOOD HO+ HOEN Weak Base Strong Acid IOH + HO'HN NH.OH + CH.COOH Weak Base Weak Acid 4. Explain why the titrations which began with CH3COOH started from a higher pH value compared to those which began with HCI. 5. What was the purpose of adding the indicator to each titration? 6. Two titrations ended with the pH well above 10 the other two titrations ended with the pH below 10. Explain why this occurred.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A buffer solution is prepared by mixing 20.0 mL 0.45 M CH3COOH (acetic acid) with 35.0 mL 0.45 M CH3COONa (sodium acetate) What is the amount of 4.0 M CH3COOH which must be added to this buffer solution to double the [H3O+]? What is the amount of 2.0 M HCl that must be added to decrease the pH by 0.50? How much NaOH(s) in g (grams) has to be added to the solution to raise the pH by 2.00?
QUESTION 10 Which of the following is TRUE? OA. An indicator is not pH sensitive. OB. The equivalence point is where the amount of acid equals the amount of base during any acid-base titration. OC. At the equivalence point, the pH is always 7. OD. A titration curve is a plot of pH vs. the [base]/[acid] ratio.
In an acid-base titration, 24.93 mL of an NaOH solution are needed to neutralize 16.07 mL of a 0.0643 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: a. First note the value of M+ in the HCl solution. M b. Find MOH in the NaOH solution. Mg+ x Vacid = MH- x Vosse Мон M с. Obtain Myaoн from Mон. MNAOH M
Q 25 mL of a mixture of NaOH and Na 2 CO 3 was titrated with 0.1 HCI using phenolphthalein indicator required 25 mL HCI. The same volume of mixture when titrated with O.1 N HCI using methyl orange indicator required 30 mL of HCI. Calculate the amount of Na 2 CO 3 and NAOH in one „litre of this mixture
Which of the following titrations result in an acidic solution at the equivalence point? CH3COOH + Ba(OH)2 HF + Ca(OH)2 HBr + NaOH CH3NH2 + HI
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.40 M NaH2PO4 and 0.60 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. Calculate the pH of the phosphate buffer solution? Provide your answer to 2 decimal places If the pH calculated in b was the blood pH of an actual patient, would you say this patient’s blood pH is within normal range or are they suffering from alkalosis or acidosis?
15. A buffer is prepared by mixing 2.50 g of benzoic acid (HC7H5O2) and 3.50 g of sodium benzoate (NaC7H5O2) in 1.00 L of water. The Ka for benzoic acid is 6.6 × 10-5 a. Find pH of buffer b. Find the pH of the buffer when 5.0 mL of 0.120 M HCl is added c. Find the pH of the buffer when 90.00 mL of 2.100 M HCl are added. Show all work and ICE table if applies.
A 4.50-g quantity of a diprotic acid was dissolved in water and made up to exactly 225 mL. Calculate the molar mass of the acid if 25.0 mL of this solution required 10.5 mL of 1.00 M KOH for neutralization. Assume that both protons of the acid were titrated. g/mol
The Ka of hydrocyanic acid (HCN) is 4.0 × 10-10. Determine the pH of a 0.300 mol/L solution of hydrocyanic acid. [3 T] 1. What is the pH at the equivalence point if 25.00 mL of the hydrocyanic acid is titrated with 0.300 mol/L NaOH.
At which point in the titration curve below is a buffer present? C Volume titrant added (mL) A. Ο Ρoint A В. О Рoint B C. O Point C D. O Point D E. OA buffer is not present at any point during this titration.
A titration is carried out for 25.00 mL of 0.100 M HCI (strong acid) with 0.100 M of a strong base NaOH (the titration curve is shown in Figure 14.18) Calculate the pH after the addition of 30.00 mL base.
Suppose you want to make a buffer with a pH of 6.90. Which of the following acid/conjugate base pairs should you choose? Group of answer choices HOCl and OCl- (Ka = 3.5 x 10-8) HSO4- and SO42- (Ka = 1.2 x 10-2) C6H5CO2H and C6H5CO2- (Ka = 6.5 x 10-5) HF and F- (Ka = 6.6 x 10-4)