A chemist prepares a solution of aluminum chloride (AlCl,) by measuring out 20. umol of aluminum chloride into a 250. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's aluminum chloride solution. Round your answer to 2 significant digits.

I Part 2 Procedure, Data & Analysis: Recall: The amount of ionization or dissociation of ions determines the strength of an acid or base. The concentration of [H3O+], hydronium ion and [OH]. hydroxide ion, can be used to calculate pH and pOH as shown on the diagram here: Note: we use [H3O+] and [H*] interchangeably. 1. Click on Water Solution, Graph View, Probe Tool. Insert the probe in the water. Notice that given before 2. Fill in the hydronium the the pH. 3. Use the the pOH. Equilibrium Concentration (mol/L) 10² 10¹ 10⁰ 10¹ 10 10ª 104 10% 10⁰ 107 10⁰ pH: 7.00 2 H₂O H3O+ + OH- H 1L 4 [H₂O*] or [H*] pH (OH)-1x10¹4 H (H)-1x10-¹4 -LOUISE POH-14-PH pH-14-POH Show work: [OH] LIO - امي the initial concentration of the solution is any ionization or dissociation takes place. 4. Did your answer to # 2 match the pH given in the simulation? 5. Is the answer to #3 equal to: (14 - pH)? 6. Is the solution an acid, a base or neutral, based upon the calculated pH? Attach notebook paper to show…

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all 43% LTE 2:34 Question 4 of 8 Submit Construct the expression for Ka for the weak acid, NH,*. NH,*(aq) + H,0(10) = H,0*(aq) + NH;(aq) 1 Based on the definition of Ka, drag the tiles to construct the expression for the given acid. Ka %3D 5 RESET [H,O] [H,O*] [OH-] [NH,] [NH,] [NH,] 2[H,0O] 2[H,0*] 2[OH-] 2[NH,] 2[NH,] 2[NH,] [H,0]? [H,0*12 [OH-]? [NH,*)? [NH,]? [NH,-]? II