SET-1 1. Acids produce; when dissolved in water. a. Na+ ions b. OH ions c. H+ ions d. Cl ions 2. A solution with a pH of 4 is; a. Neutral b. Acidic c. Basic d. Salty 3. H2SO4 is added to the oxalic acid solution before titration with KMnO4 solution to: Speed up reaction a. b. Slow down reaction c. d. Dissolve formed ions Help produce a color at the endpoint. 1. A solution with a pH of 7 is SET-2 a. Neutral b. Acidic c. Basic d. Salty 2. Bases produce;. when dissolved in water. a. Na+ ions b. OH- ions c. H+ ions d. Clions 3. For bases, the following is true. a. [H+] = [OH] b. [H+] > [OH] c. [H+] < [OH] d. [OH-] is zero

I The endpoint of an acid-base titration is defined as the point where O A. The amount (moles) of acid and base present are equivalent and a physio-chemical change occurs. O B. All the base added from the burette is used up. O C. Excess titrant is present. O D. The number of moles of acid and base are equal.

1.  Define the following terms used in volumetric/ titrimetric analysis       a.   Standard solution       b.   Titrate/titrand/analyte       c.   Titrant       d.   Endpoint       e.   Equivalence point       f.   Indicator       g.   Titration       h.   Titration error 2.  What are the types of volumetric/titration method? Define each.

4. Describe the pH changes as large or small in the vicinity of the: Titration of 10 ml. of an a. equivalence point pll b. half-equivalence point 5. Refer to the figure to answer the questions a & b. a. What is the pk, of the unknown acid? b. What is the K, of the unknown acid? 6. Two unknown, weak, monoprotic acids of equal concentration were titrated separately with NaOH. Upon evaluation, the titration curves revealed that the pk, of Acid 1 is 8.1 and the pk, of Acid 2 is 5.8. • s0 100 150 200 al. ef00M NuOl added Which acid is the stronger acid?

Direction: Choose the best answer. 1. The concentration of the unknown substance in titration is determined by what measure? A. molality B. molarity C. ppm D. ppb 2. By what type of solution can you categorize a solution whose concentration or strength has been correctly established is a standard solution? A. basic B. inorganic C. organic D. standard 3. What is point in titration which it is determined by the use of an indicator which changes color at the desired point? A. Acid point B. basic point C. equivalence D. turning 4. What is being avoided in cleaning the laboratory tools and equipment before using? A. contamination B. errors C. fire D. viruses 5. A burette is used to dispense unknown liquid into the flask. What part of the burette is responsible in stopping the flow of liquid in it? A. funnel B. pinchcock C. nozzle D. opening 6. For any chemical reaction carried out in any manner, the quantity of heat absorbed or evolved by the reaction is…

3. A 50.0 ml of 0.02 F ammonia solution is added to a solution containing 0.004 g Ni?, 0.003 g Mn. and 0.002 g Cra per 750 ml. a. calculate whether or not a precipitate wil torm b. it answer to (a) is yes, formulas of precipitates c. which ion wil precipitate frst d. what pH is necessary to prevent precipitation of all cations

I. True or False 1. Strong acids are acids with high concentration. 2. The solubility of PbCl, decreases in a solution that contains both PbCl, and NaCl. 3. PBSO, will precipitate from a solution containing 1.5 x 103 M Pb(NO,), and 0.05 M Na,SO̟. 4. All acids and bases have conjugates. 5. Blood uses a buffer bicarbonate ions and carbonic acid. II. The product of [H3O+] and [OH-] in water a. is greater than 1 b. decreases with pH c. increases with pH d. is kw, the ion product constant

21. What materials contain a precisely known concentration of a substance typically used in quantitative analysis?   A. ACS grade MaterialsB. Chemical Standard MaterialsC. IUPAC Standard MaterialsD. PIPAC Standard Materials22. Which type of curve is normally produced when plotting the change in the concentration of a specie of some function and the amount of reagent added?A. Titration curveB. Sigmoidal CurveC. Phase Transition curveD. Calibration curve23.In the dead dear case study, silver diethyldithiocarbamateforms a colored solution when it binds with arsenic, what do we call substance like silver diethyldithiocarbamate?A. Secondary standard reagentB. Precipitating agentC. Chelating agentD. Primary standard reagent24.What important analytical method is employed that include analysis of standard reference materials when available, analysis by a different analytical method, analysis of “spiked” samples, and analysis of synthetic samples approximating the chemical composition of the…

6:07 LTE 74 Ch 17 Buffers and solubility 1. Buffers: C... 2. Buffers: C... M 3. Buffer P... 1req 4. Titration C... M 1req 5. Titration... Preparation Question [Review Topics] The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a monoprotic base. Question Question 6. Writing Ksp... 7. Ksp: Calcul... 6 M 4 8 2 0 M M 8. Common I... 5 10 15 20 25 30 35 40 45 50 mL of 0.1 M base added 9. Precipit... 1req (1) The pH curve M 10. Buffer + represents the titration of a with a ✰ acid Progress: 7/10 groups Due Apr 12 at 10:00 PM base. (2) Choose a Previous Next Finish Assignment Email Instructor Save and Exit Αν 03-cnow-owl.cengagenow.com ?

11. What effect will addition of excess of HCI have on the pH of a solution of NH3? a. increase the pH b. decrease the pH C. no effect d. cannot tell from information given > Answer and brief explanation: 12. A buffer solution may be a mixture of a. a weak acid and its salt b. a weak base and its salt C. an excess of a weak acid with a strong base d. all of the above > Answer and brief explanation: 13. The ammonium ion would be classified as a Bronsted a. acid b. base > Answer and brief explanation: