Determine the pH of a solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 NEXT > A solution is prepared with 0.075 M (CH3)³N and 0.10 M (CH3)NHCI. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2x 0.10-2x (CH3)3N(aq) + 0 0.075 + x 0.075 0.075-x 0.10 2 H₂O(l) 0.075 + 2x 5.2 x 10- 0.075 - 2x +x OH (aq) 0.10 + x -X 0.10-x + (CH,),NH*(aq) RESET +2x 0.10+2x
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- A solution of sodium acetate is prepared using 0.56 mol L-1 NaOH as the solvent. The pKapKa of acetic acid is 4.75 . The concentration of sodium acetate after mixing, before any reaction takes place is 0.44 mol L-1 . Calculate the equilibrium concentrations of all acid species: [ CH3COOH ], [ CH3COO- ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correct assumptions first, the quadratic formula will give you the wrong answer. [ CH3COOH ] = ___mol L-1 , [ CH3COO- ] = ___mol L-1 , pH = ___ pOH = ____In solutions 1-4 you are adding successively larger volumes of 0.00200 M SCN- to the Fe3+ solution and diluting to 10.00 mL. Calculate the final diluted molarity of SCN- in solution #1. 3 sig figs (Calculate the same thing for the solutions 2-4 and enter the results in table 3 as [SCN-] pre-equilibrium.)A 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.
- Q1.0 When 0.39 mol of solid CO2 is reacted with 0.23 mol of CH3MgBr in an ether solvent, the resulting product is isolated in aqueous solution (assuming 100% yield) and any excess CO2 is removed. Following this, 0.13 mol of HCl (aq) is added. What is the resulting solution's pH? Please note that you will need to research a pKa value for this query, and your answer should be reported to two decimal points.Acetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions: HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone protons, H+ (aq), do not exist!). (a) Write the equilibrium constant expression for the dissociation of acetic acid. (b) Vinegar sold commercially is typically 0.8 − 1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures? (c) What is the value of the equilibrium constant Keq for the dissociation according to the concentrations from part (b)? (d) When starting with completely un-dissociated…What are the factors that affect buffer capacity? Explain in 2-3 sentences.
- For acid solutions comprised of a moderately concentrated mixture of strong and weak acids, the [H+] concentration is approximately equal to the concentration of the strong acid (e.g. HNO3). This approximation applies to the acid rain experiment you are about to carry out. In your experiment, acid rain samples will involve the following reactions: weak acid : HNO2 H + + NO− strong acid : HNO3 ⎯ → H + + NO− From these reactions, you can recognize that the strong acid, nitric acid, completely dissociates into hydrogen ions and nitrate ions, whereas the weak acid, nitrous acid, is predominately in its molecular form, HNO2. B. The total acid concentration (nitric + nitrous acid) of the 10.0 mL solution of “acid rain” is determined by an acid-base titration method. You add 5.00 mL of the titrant sodium hydroxide with a concentration of 0.0114 M to reach the endpoint. i. What is the number of moles of hydroxide ions added? ii.Write one net ionic equation for the…For acid solutions comprised of a moderately concentrated mixture of strong and weak acids, the [H+] concentration is approximately equal to the concentration of the strong acid (e.g. HNO3). This approximation applies to the acid rain experiment you are about to carry out. In your experiment, acid rain samples will involve the following reactions: weak acid : HNO2 H + + NO− strong acid : HNO3 ⎯ → H + + NO− From these reactions, you can recognize that the strong acid, nitric acid, completely dissociates into hydrogen ions and nitrate ions, whereas the weak acid, nitrous acid, is predominately in its molecular form, HNO2. A. One simple way to measure the [H+] is to measure pH. If a 10.0mL solution of “acid rain” is measured to have a pH=2.77, what is the concentration of strong acid, HNO3, formed? Hint: pH=-log[H+] and 10–pH= [H+], where [H+] is in molarity units.A solution is made by mixing exactly 500 mL of 0.156 M NaOH with exactly 500 mL of 0.100 MCH3COOH. Calculate the equilibrium concentration of the species below. Ka of CH3COOH is 1.8×10−5 [H+] M Enter your answer in scientific notation. [OH−] M [CH3COOH] M Enter your answer in scientific notation. [Na+] M [CH3COO−] M
- Complete the following: 1. Random error, also called _________arises from the effects of uncontrolled variables in the measurement. 2. The ____________,measures how closely the data are clustered about mean. 3. The chemical equilibrium in which all the reactants and products are in the same phase are called____________. 4. Reaction that go to completion and never proceed in the reverse direction are said to be_____________ 5. The equation for buffer is the__________equation. 6. A ___________solution is one that resists changes in pH when small quantities of an acid or an alkali added to it. 7. __________is the pH of the pure, neutral and polyproticNitrous acid (HNO2) is an essentially nonvolatile acid that ionizes in water with an equilibrium constant of 4 x 10-4 mol/liter. Assume that 10 mmol of nitrous acid are added to a liter of water that is open to the atmosphere.a. List all chemical species that you expect to occur in the water. For which of these do you know the concentration a priori? (you may assume the water has reached equilibrium with the air, and therefore H2CO3* concentration is approximately 12 mM, per Henry’s law)b. Write every equation that constrains the composition of the system at equilibrium identifying each as a mass conservation, mass action, or electroneutrality constraint.The ionization constant of a very weak acid, HA, is 1.6×10-9. Calculate the equilibrium concentrations of H3O+, A-, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] = _______ mol/L [A-] = __________ mol/L [HA] = _________ mol/L pH = ___________