Homework Answers
5. In the hood, form solid AgCl by adding 1 mL of 6 M HCI (aq) to 1 mL of 0.1 M AgNO3 (aq) in a m...
5. In the hood, form solid AgCl by adding 1 mL of 6 M HCI (aq) to 1 mL of 0.1 M AgNO3 (aq) in a medium test tube, and then add 1 drop of 15 M NH3 (aq) to establish the equilibrium shown below. AgCI (s) +2 NH3 (aq)Ag(NH3)2 (aq)+CI (aq) Stress 1. Add reactant. Stress 2. Add product. action observation shift right or left Stress 1 Stress 2 What happens to the concentration of CI as reactant is...
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine whic...
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...
A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3
1)A 10.0 mL sample of 0.25 M NH3(aq)
is titrated with 0.20 M HCl(aq) (adding HCl to
NH3). Determine which region on the titration curve the
mixture produced is in, and the pH of the mixture at each volume of
added acid.Kb of NH3 is 1.8 ×
10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the
mixture is [ Select ] ["at", "before", "after"] the
equivalence point on the titration curve.2) The pH of the solution after...
Calculate the pH after adding 0.5 mL of 0.1 M HCl to 100 mL of a...
Calculate the pH after adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H2PO, ] = [HPO? 1=0.35 M? What will be the effect on the initial pH? 3 Part I: Preparation of acetate buffer solution (20 points) Solution Initial pH After adding 2 ml HCI After adding 2 ml NaOH Distilled water 7.1 2.2 12.5 Acetate buffer 4.5 4.3 4.7 Determination of K of the buffer solution Calculated Concentration of CH3COOH Calculated...
1. I placed 5 mL of 0.025 M CuSO4 in a test tube, and slowly added...
1. I placed 5 mL of 0.025 M CuSO4 in a test tube, and slowly added 15 M NH3 until my solution turned blue, I then removed reactant by adding (CuSO4, NH3, H20, HCl, NaOH) and my test tube appeared clear, light light blue. That's because as I removed reactant, the Cu2+ concentration (increased, decreased, stayed the same) 2. In a medium test tube, I added 2 drops of 6 M NaOH to 5 mL of 0.05 M MgCl2(aq) to...
help please! 4. You added 0.05 mL of 0.10 M AGNO3 to 4.0 mL of 2.0...
help please!
4. You added 0.05 mL of 0.10 M AGNO3 to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s): K=Ksp Ag (aq)+ CI (aq) AgCl (s) Using this saturated solution as the test solution you set up the following cell AglAg' (test solution after reaction)||Ag* (1.0M) |Ag and measured Ecell= 0.61 V. (a) Using the measured value of Eel and Eq (15), calculate the equilibrium [Ag'] (i.e. of the test solution after reaction)....
PRELAB ASSIGNMENT (CO 4. You added 0.05 mL of 0.10 M AgNO, to 4.0 mL of 2.0 M NaCl, and formed a ...
PRELAB ASSIGNMENT (CO 4. You added 0.05 mL of 0.10 M AgNO, to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s) AgCl (s) Ag+ (aq)+ Cl-(aq) Using this saturated solution as the test solution you set up the following cell and measured Ecell = 0.61 V (a) Using the measured value of Eell and Eq (15), calculate the equilibrium [Ag'] (i.e. of AglAg' (test solution after reaction)lAg (1.0M)Ag the test solution after reaction). (1...
4. You added 0.05 mL of 0.10 M AgNO, to 4.0 mL of 2.0 M NaCl,...
4. You added 0.05 mL of 0.10 M AgNO, to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s): AgCl (s) 7 Ag+ (aq)+CF (aq) K=Ksp Using this saturated solution as the test solution you set up the following cell AgAg (test solution after reaction)||Ag (1.0M) Ag and measured Ecell = 0.61 V. (a) Using the measured value of Ecell and Eq (15), calculate the equilibrium (Ag l (i.e. of the test solution after reaction)....
Find the Qsp when 3.1 mL of 1 M HCl(aq) and 4.8 mL of 0.0026 M...
Find the Qsp when 3.1 mL of 1 M HCl(aq) and 4.8 mL of 0.0026 M AgNO3(aq) are mixed together with enough water to dilute the solution to 60 mL. The solubility product of AgCl is 1.6 × 10−10 .
i) solution made by adding 5.0 mL of 0.10 M HCl to 100 mL of a...
i) solution made by adding 5.0 mL of 0.10 M HCl to 100 mL of a buffer containing 0.15 M acetic acid and 0.15 M acetate
5. In the hood, form solid AgCl by adding 1 mL of 6 M HCI (aq) to 1 mL of 0.1 M AgNO3 (aq) in a medium test tube, and then add 1 drop of 15 M NH3 (aq) to establish the equilibrium shown below. AgCI (s) +2 NH3 (aq)Ag(NH3)2 (aq)+CI (aq) Stress 1. Add reactant. Stress 2. Add product. action observation shift right or left Stress 1 Stress 2 What happens to the concentration of CI as reactant is...
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...
1)A 10.0 mL sample of 0.25 M NH3(aq)
is titrated with 0.20 M HCl(aq) (adding HCl to
NH3). Determine which region on the titration curve the
mixture produced is in, and the pH of the mixture at each volume of
added acid.Kb of NH3 is 1.8 ×
10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the
mixture is [ Select ] ["at", "before", "after"] the
equivalence point on the titration curve.2) The pH of the solution after...
Calculate the pH after adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H2PO, ] = [HPO? 1=0.35 M? What will be the effect on the initial pH? 3 Part I: Preparation of acetate buffer solution (20 points) Solution Initial pH After adding 2 ml HCI After adding 2 ml NaOH Distilled water 7.1 2.2 12.5 Acetate buffer 4.5 4.3 4.7 Determination of K of the buffer solution Calculated Concentration of CH3COOH Calculated...
help please!
4. You added 0.05 mL of 0.10 M AGNO3 to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s): K=Ksp Ag (aq)+ CI (aq) AgCl (s) Using this saturated solution as the test solution you set up the following cell AglAg' (test solution after reaction)||Ag* (1.0M) |Ag and measured Ecell= 0.61 V. (a) Using the measured value of Eel and Eq (15), calculate the equilibrium [Ag'] (i.e. of the test solution after reaction)....
PRELAB ASSIGNMENT (CO 4. You added 0.05 mL of 0.10 M AgNO, to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s) AgCl (s) Ag+ (aq)+ Cl-(aq) Using this saturated solution as the test solution you set up the following cell and measured Ecell = 0.61 V (a) Using the measured value of Eell and Eq (15), calculate the equilibrium [Ag'] (i.e. of AglAg' (test solution after reaction)lAg (1.0M)Ag the test solution after reaction). (1...
4. You added 0.05 mL of 0.10 M AgNO, to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s): AgCl (s) 7 Ag+ (aq)+CF (aq) K=Ksp Using this saturated solution as the test solution you set up the following cell AgAg (test solution after reaction)||Ag (1.0M) Ag and measured Ecell = 0.61 V. (a) Using the measured value of Ecell and Eq (15), calculate the equilibrium (Ag l (i.e. of the test solution after reaction)....
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