HCl is a strong acid and it dissociates 100% completely in aqueous solutions therby produces 100% H+ ions, hence we can use formula pH = -log[H+], pH = -log[0.1] = 1
whereas HF is a weak acid it will not completely dissociates into ions (not 100%) in aqueous solutions, hence we use Ka, dissociation constant which is different for every weak acid. for HF Ka = 7.2 X 10-4 now we have to use formula
[H+] = sqrt( Ka X C)
[H+] = sqrt ( 7.2 X 10-4X 0.1) = 8.5 X 10-3
pH = -log[H+] = -log[8.5 X 10-3] = 2.1
A 0.1 mol/L hydrochloric acid solution has a pH of 1.0 while a 0.1 mol/L hydrofluoric...
Post Lab Activity Acids, Bases, pH, and Buffers 1. Calculate the pH of a 0.08 M NaOH solution. 2. Hydrochloric acid is a strong acid and dissociate almost 100% in aqueous solution. If two drops (0.1 mL) of 1.0 MHCI are added to pure water to make 1.0 L solution. What is the pH of this solution? 3. M. What will be the A dilute solution of hydrochloric acid (HCI) has a concentration of 0.1 pH of this solution? 4....
3. A dilute solution of hydrochloric acid (HC) has a concentration of 0.1 pH of this solution? a concentration of 0.1 uM. What will be the Ce Window ng to another question will save the response Question 3 of 20 Question 3 5 points Save A Provide an appropriate response Ange des reticeThe set of 35 equally likely outcomes is 1.21.1.31.4 (L.) (L 2.11 2.2 2.3 2.412.51 (26), 3.110.210.310.401.06.14. 11.04.2014 31 4 6 5 1 5611811621631641651661. Find the probability of...
pH [H3O+] [OH−] 0.1 L solution 2.5 3.2*10^-3 3.2*10^-12 1.0 L solution 3.50 3.2*10^-4 3.2*10^-11 Find the product of the [H3O+] and the [OH−] for the 0.1 L solution. Find the product of the [H3O+] and the [OH−] for the 1.0 L solution. Select the statement that best answers the following question What is the relationship between [H3O+] and [OH−] for the solutions? The product of [H3O+] and the [OH−] is greater for a solution with a higher pH. The...
A. Hydrochloric Acid Solution and pH 1. Write the balanced chemical reaction for the dissociation of the hydrochloric acid. 2. Refer to the procedure for A to determine the concentrations of the solutions of hydrochloric acid. Remember to use MiV1-MV. Show work for trial 1. 3. Calculate the theoretical pH of each hydrochloric acid solution. Recall that hydrochloric acid is a strong acid, suggesting complete dissociation, so that the equation pH log (HO) can be used (equation 3). Show work...
a. How would you prepare a buffer with pH 3.00? Answer: mix 1.0 mol hydrofluoric acid with 0.71 mol sodium fluoride in 1.0 L water. b. If you add 0.010 mol HCl to the buffer in 5a, calculate its pH. Answer: pH = 2.99 c. If you add 0.010 mol HCl to 1.0 L water, what is the pH? Answer: pH = 2.00
Dissociation Ethanoic Acid Hydrochloric Acid Nitric Acid Phosphoric Acid Universal solution Universal chart (enter label here) pH Meter Dissociation 1- Follow the dissociation experiment procedure and answer the following questions. 2- Identify which of these acids which are provided in the experiment are strong acids or weak acids and why? (look at the reaction details bax) By using the pH universal chart and solution 3- Write down the pH value for each acid. 4- Does 1 M of strong acid...
Hydrofluoric Acid has a dissociation constant at 25°C of 6.7 x10-4. If 1.0 mol of HF is dissolved in enough water to give 1.00 L of solution, what is the hydrogen ion concentration in this solution expressed in M? a) 2.0 x 10-2 b) 2.6 x 10-2 c) 3.3 x 103 d) 6.7 x 10-4 e) none of the above Оа Od Ob Ос
I. REACTION EQUILIBRIUM IN NON-IDEAL SYSTEMS The acetic acid (CH:COOH) aqueous solution with a concentration of 0.1 mol/kg has a hydrogen ion concentration of 1.35x10-3 mol/kg. i. Write the acid dissociation equation. ii. Calculate the acid dissociation constant, Ka, considering the ionic activity. jïi. Calculate the pH of the acidic solution. iv. What is the new pH if the solution contains 0.1 mol CH3COOH and 0.4 mol of sodium acetate, CH3COONa, in 1.0 L of water? Consider the negligible quantitities....
Consider the following data on some weak acids and weak bases: acid name hydrofluoric acid formula HF 6.8 x 10-4 base name formula hydroxylamine HONH2 1.1 x 10-8 ammonia NH, 1.8 10-5 hydrocyanic acid HCN 4.9 x lo-10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution tha the solution that will have the next lowest pH, and so on. solution PH 0.1 M HONHJCI choose...
Consider the following data on some weak acids and weak bases: acid name formula hydrofluoric acid HF 6.8*10-4 HNO2 4.5 x 104 base к, name formula pyridine C,HN 1.7 x 10-2 hydroxylamine HONHX 1.1 x 10-8 nitrous acid Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH,...