QUESTION 1
Which of the following solutions is a buffer?
A mixture of HF and HBr |
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A mixture of H2SO4 and Na2SO4 |
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A mixture of NaI and HI |
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A mixture of NaF and HF |
1 points
QUESTION 2
What is the [A-]/[HA] ratio in a buffer made of HA and its conjugate base, A-, and has a pH of 8.00 ? The pKa of HA is 6.00
1:1 |
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1:10 |
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1:100 |
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10:1 |
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100:1 |
1 points
QUESTION 3
3[Mg2+] = s |
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[Mg3+] = 2s |
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[Mg2+] =3s |
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[PO43-] =3s |
1 points
QUESTION 4
A solution mixture contains equal concentrations of Cl-, I- and Br- ions. If a dilute solution of Ag+ ions is slowly added to the mixture, what is the correct order with which the precipitates will form?(from first to last in precipitation) Ksp of : AgCl =1.8 ×10-10, AgBr =5.0 ×10-13 , AgI = 8.3 ×10-17
AgCl,AgBr, AgI |
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AgI,AgCl,AgBr |
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AgCl,AgI, AgBr |
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AgI,AgBr,AgCl |
1 points
QUESTION 5
Methyl orange is an indicator with Ka= 1.0× 10-4. Its acid form is red while its dissociated form is yellow. When it is used for a titration of aniline with HCl (HCl in buret) which has a pH at equivalence point 4.6 , what is the color change at endpoint.?
red to yellow |
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yellow to red |
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colorless to red |
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yellow to colorless |
1 points
QUESTION 6
The pH at equivalence point in a titration was found to be below 7.00 ( <7.00).Which of the following titration will it be?
Weak base vs strong acid |
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Strong base vs strong acid |
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Strong acid vs strong base |
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Weak acid vs strong base |
1 points
QUESTION 7
The reaction, A + B → C + D has a rate law expression as rate = k[A]2B. If the concentration of B is doubled (assume concentration of A is unchanged) the rate of the
reaction _______.
will decrease to half. |
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will be four times |
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will double |
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will be four times |
1 points
QUESTION 8
The reaction, 2A + B + 3C → 2X + Y is found to be zero order with respect to A, second order with respect to B and first order with respect to C. Which of the following is the correct rate law for the reaction?
k= rate[B]2[C] |
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rate= k[B]2[C] |
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rate= k[A][B]2[C] |
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rate = k[A]2[B][C]3 |
1 points
QUESTION 9
A 25.00 mL sample of 0.2000 M hypochlorous acid (HOCl, Ka = 2.9 × 10-8) is titrated with 0.2500 M KOH. What would be the pH at equivalence point?
4.25 |
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10.29 |
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3.71 |
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9.30 |
2 points
QUESTION 10
8.3 × 10-5 |
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5.2× 10-8 |
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3.2× 10-4 |
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1.9× 10-7 |
2 points
QUESTION 1 Which of the following solutions is a buffer? A mixture of HF and HBr A...
EXP #9:Pre-Lab answer question 3, attached below is page two to reference! Instructor Name: Student Name: 3. An unknown solution gives the following sequential results for color when indicators are added (shown below). Using the corresponding color ranges from the table on page 2, estimate the approximate pH range of this unknown solution. Explain. Bluish purple Bromphenol blue: Yellow Methyl Red: Blue Bromothymol Blue: Colorless Phenolpthalein: For a titration, pure indicators are used because the goal is to use an...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is to indicate the of the titration. Use Table 10.2 for the following question. If an acidic solution is titrated with a basic solution and methyl violet is used as an indicator, the solution color will change from to QUESTION 2 3 points Save Answer The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCI (aq) in 133 mL of water...
Mark each of the following statements about the ½ equivalence point of an acid-base titration TRUE or FALSE. a. It is the point in the titration when the concentration of weak acid (HA) being titrated is equal to the concentration of the conjugate base (A− ). b. It is the point halfway between the beginning of the titration of a weak acid or weak base and the equivalence point. 2 c. When a strong acid is titrated with a strong...
Question 50 1 Which of the following combinations would have a titration curve starting at pH = 10.7 and an equivalence point at pH = 4.5? Weak acid to which strong acid is added Weak base to which strong base is added Strong acid to which strong base is added Strong base to which strong acid is added Weak base to which strong acid is added
QUESTION 1 pH = 7 at the equivalence point of the titration of: O a. Weak acid with strong base. Ob.Strong acid with weak base. O C. Strong acid with strong base. Od. Weak acid with weak base.
1. The following pictures represent solution at various points in the titration of a weak acid with a strong base. HA + OH - HOH + A OH - -OH Which picture to the left corresponds to cach of the following points in the titration? before the addition of any NaOH at the equivalence point where only a salt remains which solution is a buffer? Multiple Choice 1. Barium hydroxide is slightly soluble in water, with a Kap of 5.00...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water and titrated against 0.1555 M NaOH, requiring 48.11 mL to of NaOH to reach the end-point. During the titration reaction, the pH of the solution is 3.77 when half of the HA is neutralized and the equivalence-point pH is 8.33. (a) State two ways to standardize the NaOH used in the titration. (b) Suggest and explain an indicator that can be used in the...
please help me plot/ and draw the curve (ph, pka, and equivalence ph value) α= 0.0 6. Sketch a plot below of a titration curve (pH vs volume of NaOH) when 25 mL of a 0.10N weak acid HA (Ka 1.00 X 10 is titrated with 0.10N strong base NaOH Indicate on the plot the initial pH, pha, 10% and 90% equivalence, equivalence, and final pH yalues. α= 0.0 6. Sketch a plot below of a titration curve (pH vs...
15. A 66 mL sample of a solution of sulfuric acid, H,SO, is neutralized by 34 mL of a 0.13 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution 16. If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? 17. If 287 mL of 4.7 M HCl solution is added to 284 mL of 3.2 M Ba(OH), solution, what will the pH be? 18. What is...
Which is true for the following titrations. Question 3 options: 123 The titration of a strong base using a strong acid. 123 The titration of a weak base using a strong acid. 123 The titration of a weak acid using a strong base. 1. The pH at the equivalence point is approximately equal to 7.0. 2. The pH at the equivalence point is less than 7.0 3. The pH at the equivalence point is greater than 7.0. Question 4 (1...