Homework Answers
Upon dilution , pH of the buffer solution remains same
It doesn't change much so upon dilution 10 fold ( or a factor of 10 ) , pH of buffer remains unchange . The pH of the diluted buffer will be 6.2 only.
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A pH 6.2 buffer is diluted by a factor of 10 by placing 10mL of the...
What are the concentration of this following solutions 1. 5mL of 10ppm Fe+2 diluted in a 100mL volumetric flask 2. 10mL...
What are the concentration of this following solutions 1. 5mL of 10ppm Fe+2 diluted in a 100mL volumetric flask 2. 10mL of 10ppm Fe+2 diluted in a 100mL volumetric flask 3. 20mL of 10ppm Fe+2 diluted in a 100mL volumetric flask 4. 25mL of 10ppm Fe+2 diluted in a 100mL volumetric flask
Using a 0.20 M phosphate buffer with a pH of 6.2, you add 0.77 mL of...
Using a 0.20 M phosphate buffer with a pH of 6.2, you add 0.77 mL of 0.45 M HCl to 48 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) Using a 0.20 M phosphate buffer with a pH of 6.2, you add 0.77 mL of 0.45 M NaOH to 48 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
A buffer solution is prepared by placing a 25.00 mL aliquot of 0.165 M NH3 and...
A buffer solution is prepared by placing a 25.00 mL aliquot of 0.165 M NH3 and a 25.00 mL aliquot of 0.150 M NH4Cl into a 100.00 mL volumetric flask and diluting to the mark. Using activities, calculate the pH of the buffer solution. Use the Davies equation to determine activity coefficients. (pKa of NH4+ = 9.245)
Please ans as soon as possible 0.1 M Phosphate Buffer PH 6.6 a)10ml +200ul in HCL...
Please ans as soon as possible 0.1 M Phosphate Buffer PH 6.6 a)10ml +200ul in HCL b)10ml+200ul in NaOH a)Beaker#1 b)Beaker#2 PH-6.6 PH-6.6 After adding HCL PH-6.24 After adding NaOH PH-7.04 PH 7.6 a)10ml +200ul in HCL b)10ml+200ul in NaOH a)Beaker#1 b)Beaker#2 PH-7.6 PH-7.6 After adding HCL PH-7.04 After adding NaOH PH-10.19 PH 8.6 a)10ml +200ul in HCL b)10ml+200ul in NaOH a)Beaker#1 b)Beaker#2 PH-8.6 PH-8.6 After adding HCL PH-7.24 After adding NaOH PH-11.00 1.0 M Phosphate Buffer PH 7.6 Beaker...
Phosphoric acid is a triprotic acid (K -69 x 10-M K2 - 6.2 x 10-M, and...
Phosphoric acid is a triprotic acid (K -69 x 10-M K2 - 6.2 x 10-M, and K = 48 x 10- M). To find the pH of a buffer composed of H, PO, (a) and HPO(a), which pk, value would you use in the Henderson- Hasselbalch equation? Opk1 = 2.16 Opka = 7.21 pk = 12.32 Calculate the pH of a buffer solution obtained by dissolving 24.0 KH PO(S) and 41:0g Na, HPO(s) in water and then diluting to 1.00L...
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-, K2 = 6.2 x 10...
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-, K2 = 6.2 x 10 %, and Kj] = 4.8 x 10-1). (aq), which pK, value should be used in the To find the pH of a buffer composed of H,PO] (aq) and HPO Henderson-Hasselbalch equation? OPK 1 = 2.16 OPK 2 = 7.21 Opka = 12.32 Calculate the pH of a buffer solution obtained by dissolving 11.0 g of KH, PO (s) and 21.0 g of Na, HPO...
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, Ka2 = 6.2 x 10-8,...
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To find the pH of a buffer composed of H,PO, (aq) and HPO2 (aq), which pKa value should be used in the Henderson-Hasselbalch equation? O pK al = 2.16 OpKq2 = 7.21 O pK a3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 19.0 g of KH,PO4(s) and 30.0 g of Na, HPO4(s) in...
Should the pH of a buffer change when the buffer is diluted? Explain fully, using the Henderson-H...
please help me answer those 3 questions!!
Should the pH of a buffer change when the buffer is diluted? Explain fully, using the Henderson-Hasselbalch equation as wel as your results from Solutions 10 and 11 c. pH calculation for Solution 13 pH calculation for Solution 14 Sol'n Composition 15 mL CH3COOH 2 10 mL CH3COOH+10 mL H20 3 1 mL CH3COOH + H20 to make 100 mlL 4 10 mL CH3COOH +10 mL HCI 5 H3PO4 6 7 8 10...
Phosphoric acid is a triprotic acid (Kai 6.9 x 10-3, K, -6.2 x 10-8, and Ks...
Phosphoric acid is a triprotic acid (Kai 6.9 x 10-3, K, -6.2 x 10-8, and Ks -4.8 x 10-13). To find the pH of a buffer composed of H,PO (aq) and HPO? (aq), which pK, value should be used in the Henderson-Hasselbalch equation? O pK,i 2.16 。pK2 7.21 〇pKg = 12.32 Calculate the pH of a buffer solution obtained by Jissolving 17.0 g of KH2PO,(8) and 33.0 g of Na, HPO,(s) in water and then diluting to 1.00 L pH...
If a buffer solution is 0.240 M in a weak acid Ka=6.2×10−5) and 0.420 M in...
If a buffer solution is 0.240 M in a weak acid Ka=6.2×10−5) and 0.420 M in its conjugate base, what is the pH?
Phosphoric acid is a triprotic acid (K -69 x 10-M K2 - 6.2 x 10-M, and K = 48 x 10- M). To find the pH of a buffer composed of H, PO, (a) and HPO(a), which pk, value would you use in the Henderson- Hasselbalch equation? Opk1 = 2.16 Opka = 7.21 pk = 12.32 Calculate the pH of a buffer solution obtained by dissolving 24.0 KH PO(S) and 41:0g Na, HPO(s) in water and then diluting to 1.00L...
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-, K2 = 6.2 x 10 %, and Kj] = 4.8 x 10-1). (aq), which pK, value should be used in the To find the pH of a buffer composed of H,PO] (aq) and HPO Henderson-Hasselbalch equation? OPK 1 = 2.16 OPK 2 = 7.21 Opka = 12.32 Calculate the pH of a buffer solution obtained by dissolving 11.0 g of KH, PO (s) and 21.0 g of Na, HPO...
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To find the pH of a buffer composed of H,PO, (aq) and HPO2 (aq), which pKa value should be used in the Henderson-Hasselbalch equation? O pK al = 2.16 OpKq2 = 7.21 O pK a3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 19.0 g of KH,PO4(s) and 30.0 g of Na, HPO4(s) in...
please help me answer those 3 questions!!
Should the pH of a buffer change when the buffer is diluted? Explain fully, using the Henderson-Hasselbalch equation as wel as your results from Solutions 10 and 11 c. pH calculation for Solution 13 pH calculation for Solution 14 Sol'n Composition 15 mL CH3COOH 2 10 mL CH3COOH+10 mL H20 3 1 mL CH3COOH + H20 to make 100 mlL 4 10 mL CH3COOH +10 mL HCI 5 H3PO4 6 7 8 10...
Phosphoric acid is a triprotic acid (Kai 6.9 x 10-3, K, -6.2 x 10-8, and Ks -4.8 x 10-13). To find the pH of a buffer composed of H,PO (aq) and HPO? (aq), which pK, value should be used in the Henderson-Hasselbalch equation? O pK,i 2.16 。pK2 7.21 〇pKg = 12.32 Calculate the pH of a buffer solution obtained by Jissolving 17.0 g of KH2PO,(8) and 33.0 g of Na, HPO,(s) in water and then diluting to 1.00 L pH...
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