Please correct answer and don't use hand rating Thinking (20T)1. Calculate AH for the reaction 2 Al (s) + 3 Cl₂ (g) --> 2 AICI 3 (s) from the data.(5marks)2 Al (s) + 6 HCI (aq) --> 2 AICI, (aq) + 3H2(g)HCI (g) -> HCI (aq)H2 (g) + Cl2 (g) --> 2 HCI (g)AICI, (s)--> AICI, (aq)ΔΗ = - 1049. ΚΙAH = -74.8 kJΔΗ = - 1845. ΚΙΔΗ = -323. ΚΙ

We are supposed to make the equation: 2Al(s) + 3Cl2(g) --> 2AlCl3(s)by rearranging the following…

Answered: Thinking (20T) 1. Calculate AH for the…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.32QAP

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Calculate the pH of a 1.25 L carbonate buffer which was prepared by mixing 0.1170 M of Na2CO3 and 0.400 M NaHCO3. (Ka of HCO3- = 4.70 x 10-11) pH 9.2 pH 10.8 pH 10.2 pH 9.8
5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
Important equations Attach additional paper, if necessary, to show complete work Indicate which problems you have worked out on a separate sheet of paper [HJOH)=K1.00 x 10" (at 25 "C) pH=- log (H) pOH- log (OH) pH+ pOH- 14.00 Moroo K- IHAJ ort 1. Determine the phi of 0.055 M oxalic acid (HCO, K. -5.6x 10' and K-54x 10). Note: both steps are important here, therefore we have to set up two "ICE boxes 2. Nicotine, CHN, is a base that will accept two protons (K,7x 10, K 14x 10"). What is the pH and the concentration of each species present in a 0.010 M solution of nicotine?
Calculate the pH at following volume of the acid Just letter d and e
(c) after adding 0.030_mol of HCI to 1.0 L of the buffer solution in part (a) 0.030mol [H;O*]addea Step 1. Use Stoichiometry to calculate new concentrations Concentration (M) CH;COO-(aq) + H;O*(aq) = 0.030M %3D 1.00L solution CH,COOH(aq) + H,O (1) Initial 0.40 0.030 0.40 Change Final Step 2 Set up a reaction table with the new concentrations. Concentration (M) CH,COOH(aq) + H2O(1) + CH;COO((aq) + H;O*(aq) Initial Change Equilibrium
urgent one hour please
1. A 50.0 mL solution of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 M NaOH. What is the pH after 20.0 mL of base has been added? Ka CH3COOH = 1.8 x 10-5 I attached my answer.
At 25oC, the Ka for a certain monoprotic acid HA is 6.2x10-10. What will be the Ka value for the given reaction below?1/2Ha(aq) + 1/2H2O(l) <-> 1/2A-(aq) + 1/2H3O+(aq) Choices:1.6x10-53.8x10-192.5x10-56.2x10-10
5:51 1 .ll LTE Search Question 16 of 20 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH, with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 Based on the result of the acid-base reaction, set up the unknown. ICE table in order to determine the H2NNH3*(at H2O(1) =H;O*(aq) H2NNH2(aq + Initial (M) Change (M) Equilibrium (M) RESET 0.100 0.200 0.0333 0.0667 +x -X 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x www
5. I added 0.015 M solutions of my reactants together. At equilibrium, I found a 0.008 M concentration of HPO42. (Hint: Does NOT require use of the quadratic equation) H2PO4° (ag)+ H20 m +→ H30* (ag) + HPO2°G (ag) A) What is the Ka of my solution? B) What is the pH of my solution at equilibrium?
3: Based on the ice table and Alan expression determine the ph of the solution

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