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2. The pH of a 0.100 M solution of an acid, HA, is 1.70. Calculate the...
3. What volume of 0.025 M NaOH will be required to reach the endpoint in a...
3. What volume of 0.025 M NaOH will be required to reach the endpoint in a titration with 25.00 ml of 0.10 M HCI? Show your work with units and correct significant figures. Circle your answer. 4. Calculate the molarity of a sodium hydroxide solution if 25.00 mL 0.100 M maleic acid requires 22.10 ml of NaOH to reach the endpoint. Show your work with units and correct significant figures. Circle your answer. 5. The following data were collected in...
PRE-LAB for pH titration of a Strong Acid with Base This is due before the lab...
PRE-LAB for pH titration of a Strong Acid with Base This is due before the lab begins, Name 1. Calculate the pH of the following solutions: (a) 1 M NaCl Does not dissociate in water to produce either hydrogen or nyot thus it is a neutral Sall, so 7. (b) 1 M HOAc (Ka - 1.8 x 10-5) duce either hydrogen or hyd xde ion, (c) 1 M NHOH (Kb = 1.8 x 10-5) (d) 0.1 M NaOAC (e) 0.1...
PRE-LAB for plt.titeation.ofa 5tremsAcid.wth Bast This is due before the lab begins 1. Calculate the pH...
PRE-LAB for plt.titeation.ofa 5tremsAcid.wth Bast This is due before the lab begins 1. Calculate the pH of the following solutions (a) 1 M NaC Name (b) I M HOAc (Ka-1.8 x 10-5) (c) I M NH4OH (Kb- 1.8 x 10-5) (d) 0.1 M NaOAc (e) 0.1 M NHCI 2 The pH of a 0.100 M solution of an acid, HA, is 1.70. Calculate the K? (use ICE) 2.Show your work with units and correct significant figures for all questions that...
A 0.100 molar solution of weak acid HA has pH of 2.45 What is pka? Hint,...
A 0.100 molar solution of weak acid HA has pH of 2.45 What is pka? Hint, find [H+] from pH and plug it into into ICE as 'X' HA (+H20) А" <> H30* 0.100 M 0 0 С E 0.100 - X х х solve for Ka, then pka Ka = [H30*1 [A]/[HA] 39 24 6.1 45 5.4 Consider the titration of 25.00 ml of 0.100 MHA with 25.0 0.100 M NaOH. HA +H20 --> A™ + H307 The Ka...
1. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid,...
1. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 2. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid that has been titrated to its endpoint using NaOH, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 3. What pH did you...
(ueak acid/shing base 3. Calculate the pH at the following points for the titration of 25.0 mL of 0.100 M formic acid (Ka-1.80 x 10") with 0.100 M NaOH: VNOH 0.00 mL, 15.00 mL, 25.00 mL, 40.00...
(ueak acid/shing base 3. Calculate the pH at the following points for the titration of 25.0 mL of 0.100 M formic acid (Ka-1.80 x 10") with 0.100 M NaOH: VNOH 0.00 mL, 15.00 mL, 25.00 mL, 40.00 mL. Draw a graph of pH vs. VaoH. (30 points) (b) Buffer capacity can be thought of as how well a solution resists changes in pH after a strong base/acid is added. A buffer is most effective to resisting pH changes when what...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water...
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...
1. A 0.100 M solution of the weak acid HB has a pH of 3.00. What...
1. A 0.100 M solution of the weak acid HB has a pH of 3.00. What are the [H+], [B-], and Ka for this acid? 2. A solid acid is dissolved in water. Half the solution is titrated to a phenolphthalein end point with NaOH solution. The neutralized and acid solutions are then mixed and the pH of the resulting solution is found to be 4.60. Find Ka of the solid acid. 3. Assuming your buffered solution contains acetic acid,...
What is the pH of a solution of 40.0 mL of 0.100 M acetic acid (Ka...
What is the pH of a solution of 40.0 mL of 0.100 M acetic acid (Ka = 1.8 x 10-5) after 50.0 mL of 0.100 M NaOH has been added? Calculate the concentration of dissolved Ba2+ ions when BaSO4 is added to water at 25°C. Кsp? = 1.10 x 10-10 A particular saturated solution of silver chromate (Ag2CrO4), has [Ag+] = 5.0 x 10 Mand (CrO4) = 4.4 x 10M. What is value Ksp for silver chromate? As a result...
2. Calculate the pH expected for the following monoprotic substances. a. HCl (strong acid) 0.0100 M...
2. Calculate the pH expected for the following monoprotic substances. a. HCl (strong acid) 0.0100 M 0.100 M 0.0500 M 0.00100 M b. NaOH (strong base) 0.100 M 0.0500 M 0.0100 M Experiment 4 с. НС2Н3О2 (weak acid) (Ka 1.8 x 10-5) 0.100 M 0.0500 M 0.0100 M d. K2CO3 (weak base) (K, = 2.1 x 10-4) 0.100 M 0.0500 M 0.0100 M
2. Calculate the pH expected for the following monoprotic substances. a. HCl (strong acid) 0.0100 M 0.100...
3. What volume of 0.025 M NaOH will be required to reach the endpoint in a titration with 25.00 ml of 0.10 M HCI? Show your work with units and correct significant figures. Circle your answer. 4. Calculate the molarity of a sodium hydroxide solution if 25.00 mL 0.100 M maleic acid requires 22.10 ml of NaOH to reach the endpoint. Show your work with units and correct significant figures. Circle your answer. 5. The following data were collected in...
PRE-LAB for pH titration of a Strong Acid with Base This is due before the lab begins, Name 1. Calculate the pH of the following solutions: (a) 1 M NaCl Does not dissociate in water to produce either hydrogen or nyot thus it is a neutral Sall, so 7. (b) 1 M HOAc (Ka - 1.8 x 10-5) duce either hydrogen or hyd xde ion, (c) 1 M NHOH (Kb = 1.8 x 10-5) (d) 0.1 M NaOAC (e) 0.1...
PRE-LAB for plt.titeation.ofa 5tremsAcid.wth Bast This is due before the lab begins 1. Calculate the pH of the following solutions (a) 1 M NaC Name (b) I M HOAc (Ka-1.8 x 10-5) (c) I M NH4OH (Kb- 1.8 x 10-5) (d) 0.1 M NaOAc (e) 0.1 M NHCI 2 The pH of a 0.100 M solution of an acid, HA, is 1.70. Calculate the K? (use ICE) 2.Show your work with units and correct significant figures for all questions that...
A 0.100 molar solution of weak acid HA has pH of 2.45 What is pka? Hint, find [H+] from pH and plug it into into ICE as 'X' HA (+H20) А" <> H30* 0.100 M 0 0 С E 0.100 - X х х solve for Ka, then pka Ka = [H30*1 [A]/[HA] 39 24 6.1 45 5.4 Consider the titration of 25.00 ml of 0.100 MHA with 25.0 0.100 M NaOH. HA +H20 --> A™ + H307 The Ka...
1. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 2. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid that has been titrated to its endpoint using NaOH, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 3. What pH did you...
(ueak acid/shing base 3. Calculate the pH at the following points for the titration of 25.0 mL of 0.100 M formic acid (Ka-1.80 x 10") with 0.100 M NaOH: VNOH 0.00 mL, 15.00 mL, 25.00 mL, 40.00 mL. Draw a graph of pH vs. VaoH. (30 points) (b) Buffer capacity can be thought of as how well a solution resists changes in pH after a strong base/acid is added. A buffer is most effective to resisting pH changes when what...
What is the pH of a solution of 40.0 mL of 0.100 M acetic acid (Ka = 1.8 x 10-5) after 50.0 mL of 0.100 M NaOH has been added? Calculate the concentration of dissolved Ba2+ ions when BaSO4 is added to water at 25°C. Кsp? = 1.10 x 10-10 A particular saturated solution of silver chromate (Ag2CrO4), has [Ag+] = 5.0 x 10 Mand (CrO4) = 4.4 x 10M. What is value Ksp for silver chromate? As a result...
2. Calculate the pH expected for the following monoprotic substances. a. HCl (strong acid) 0.0100 M 0.100 M 0.0500 M 0.00100 M b. NaOH (strong base) 0.100 M 0.0500 M 0.0100 M Experiment 4 с. НС2Н3О2 (weak acid) (Ka 1.8 x 10-5) 0.100 M 0.0500 M 0.0100 M d. K2CO3 (weak base) (K, = 2.1 x 10-4) 0.100 M 0.0500 M 0.0100 M
2. Calculate the pH expected for the following monoprotic substances. a. HCl (strong acid) 0.0100 M 0.100...
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