Homework Answers
5.
Correct option: C
BH3 is a Lewis acid. This means that it is an electron acceptor. In option C, BH3 is accepting electrons from NH3. Bronsted acids are proton donor. But, BH3 is not donating any proton to NH3. Hence, the Lewis acid BH3 is not acting as a Bronsted acid.
6.
Correct option: B
The point A in the diagram represent equivalence or stoichiometric point. At this point, the moles of acid is equal to the moles of base.
7.
Correct option: D
Buffer is either a solution of weak acid and its conjugate base or weak base and its conjugate acid. So, only options B and D represent buffer solutions. Between these, the buffer in option D is more concentrated. Hence, it has more buffer capacity to prevent drastic change in pH on addition of either a strong acid or a strong base.
Add Answer to:
5,6,7
5. An example of a Lewis acid which is NOT also acting as a HBronsted...
If the Ka for HCIO, is 1,0x10, what is the Kb of CIO:? A. 1.0x1014 B....
If the Ka for HCIO, is 1,0x10, what is the Kb of CIO:? A. 1.0x1014 B. 1.0x10 C. 1.0x1015 D. 1.0x10 2 Choose the list which, based on structure, puts the acids in the order of most acidic to least acidic. A. HF> HCI> HBr> III B. CCla-COOII> CCbl-COOI> CCIH-COOH> CH-coOfI C. 1ICIO>HCIO,> HCIO3> HCIO4 D. B(OH),> NII> H2O > HF Which of the following substances will produce a basic solution? A. MgCl B. Fe(NO) C. KI D. NaF 4....
I need help with questions 1,3,4,5 1.0.15 M ammonium chloride is added to a 0.05 M...
I need help with questions 1,3,4,5
1.0.15 M ammonium chloride is added to a 0.05 M solution of ammonia. How does the pH change? NHs(aq) + H2O(1) NH(aq) + OH(aq) A. pH goes up B. pH goes down C. pH does not change 2. Which of the following would make buffer system? A. a weak asid and NaCl B. a weak acident's conjugate base C. a strong acid and a weak acid D. alveak acid and a strong acid E....
6. On the diagram at the right of titration of a weak acid by a strong...
6. On the diagram at the right of titration of a weak acid by a strong base, what is represented by the point A? A. the 50:50 buffer mixture B. the stoichiometric point C. mL added base D. the buffer zone E solution of strong base 7. Which of the following has the best buffer capacity? A. 0,2 M NH /0.2 M NHẠC B. 0.5 M HCI/O.5 M KCI C. 1.0 M HCI/1.0 M NACI D. 1.0 M HCI/1.0 M...
1. The following pictures represent solution at various points in the titration of a weak acid...
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...
Which is true for the following titrations. Question 3 options: 123 The titration of a strong...
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...
Weak Acid-Strong Base Titration Date Nanse PRE-LAB OUESTIONS 1 Calculate the molarity of a NaOH solution...
Weak Acid-Strong Base Titration Date Nanse PRE-LAB OUESTIONS 1 Calculate the molarity of a NaOH solution that was used to titrate 1.2 g of potassium acid phthalate if 37.50 ml of the base were reauired to get to the end point of the titration. 2 It takes 12.45 ml. of a 0.500 M NaOH solution larity of the acid to titrate 30.0 mL of acetic acid. What is the mo- 3. Using the titration curve below, calculate the K, of...
What is the approximate pk, for the weak acid. (d) Excess hydroxide ion (c) Equivalence point...
What is the approximate pk, for the weak acid. (d) Excess hydroxide ion (c) Equivalence point pH (b) Buffer region ta) Weak acid a) Weak acid 12 14 1 8 10 Volume of NaOH (ml.) Titration curve for the titration of a weak acid with a strong base.
can someone please help me out with questions 1-5, please To add more information this was...
can someone please help me out with questions 1-5, please
To add more information this was given to me for a lab that used
a weak acid and we added a strong base through titration. We just
observed how the ph changes. Later we then used a buffer with a
weak acid to see how buffers affect ph change. These questions are
basically surrounded around those topics to help us prepare.
However, I'm kinda confused about answering them because weak...
Tutored Practice Problem 17.3.2 COUNTS Calculate pH for a weak acid/strong base titration. Close Problem Determine...
Tutored Practice Problem 17.3.2 COUNTS Calculate pH for a weak acid/strong base titration. Close Problem Determine the pll during the titration of 57.0 ml of 0.303 M formie acid (K, - 1.8*10*) by 0.303 M N OH at the following points. (a) Before the addition of any NaOH (b) After the addition of 14.0 mL of NaOH (c) At the half-equivalence point the titration midpoint) (d) At the equivalence point (e) After the addition of 85.5 mL of NaOH Check...
Consider the titration of 40.0 mL of 0.500 M NH, with 1.00 M HC a) What...
Consider the titration of 40.0 mL of 0.500 M NH, with 1.00 M HC a) What is the initial pH of the NHg(aq)? b) What is the pH halfway to the equivalence point? c) What is the volume of HCI needed to reach the equivalence point? What is the pH at the equivalence point? d) Sketch the titration curve. Label the point(s) where there is a A) a weak base B) weak acid C) Buffer D) Strong acid in excess,...
If the Ka for HCIO, is 1,0x10, what is the Kb of CIO:? A. 1.0x1014 B. 1.0x10 C. 1.0x1015 D. 1.0x10 2 Choose the list which, based on structure, puts the acids in the order of most acidic to least acidic. A. HF> HCI> HBr> III B. CCla-COOII> CCbl-COOI> CCIH-COOH> CH-coOfI C. 1ICIO>HCIO,> HCIO3> HCIO4 D. B(OH),> NII> H2O > HF Which of the following substances will produce a basic solution? A. MgCl B. Fe(NO) C. KI D. NaF 4....
I need help with questions 1,3,4,5
1.0.15 M ammonium chloride is added to a 0.05 M solution of ammonia. How does the pH change? NHs(aq) + H2O(1) NH(aq) + OH(aq) A. pH goes up B. pH goes down C. pH does not change 2. Which of the following would make buffer system? A. a weak asid and NaCl B. a weak acident's conjugate base C. a strong acid and a weak acid D. alveak acid and a strong acid E....
6. On the diagram at the right of titration of a weak acid by a strong base, what is represented by the point A? A. the 50:50 buffer mixture B. the stoichiometric point C. mL added base D. the buffer zone E solution of strong base 7. Which of the following has the best buffer capacity? A. 0,2 M NH /0.2 M NHẠC B. 0.5 M HCI/O.5 M KCI C. 1.0 M HCI/1.0 M NACI D. 1.0 M HCI/1.0 M...
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...
Weak Acid-Strong Base Titration Date Nanse PRE-LAB OUESTIONS 1 Calculate the molarity of a NaOH solution that was used to titrate 1.2 g of potassium acid phthalate if 37.50 ml of the base were reauired to get to the end point of the titration. 2 It takes 12.45 ml. of a 0.500 M NaOH solution larity of the acid to titrate 30.0 mL of acetic acid. What is the mo- 3. Using the titration curve below, calculate the K, of...
What is the approximate pk, for the weak acid. (d) Excess hydroxide ion (c) Equivalence point pH (b) Buffer region ta) Weak acid a) Weak acid 12 14 1 8 10 Volume of NaOH (ml.) Titration curve for the titration of a weak acid with a strong base.
can someone please help me out with questions 1-5, please
To add more information this was given to me for a lab that used
a weak acid and we added a strong base through titration. We just
observed how the ph changes. Later we then used a buffer with a
weak acid to see how buffers affect ph change. These questions are
basically surrounded around those topics to help us prepare.
However, I'm kinda confused about answering them because weak...
Tutored Practice Problem 17.3.2 COUNTS Calculate pH for a weak acid/strong base titration. Close Problem Determine the pll during the titration of 57.0 ml of 0.303 M formie acid (K, - 1.8*10*) by 0.303 M N OH at the following points. (a) Before the addition of any NaOH (b) After the addition of 14.0 mL of NaOH (c) At the half-equivalence point the titration midpoint) (d) At the equivalence point (e) After the addition of 85.5 mL of NaOH Check...
Consider the titration of 40.0 mL of 0.500 M NH, with 1.00 M HC a) What is the initial pH of the NHg(aq)? b) What is the pH halfway to the equivalence point? c) What is the volume of HCI needed to reach the equivalence point? What is the pH at the equivalence point? d) Sketch the titration curve. Label the point(s) where there is a A) a weak base B) weak acid C) Buffer D) Strong acid in excess,...
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