Question

You are given an HCl (strong acid) solution with a pH = 2 . If you...

You are given an HCl (strong acid) solution with a pH = 2 . If you dilute 10 mL of the solution in to a total of 100 mL, the resulting pH will be closets to? a) 1 b) 2 c) 3 d) 4 e) 5

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
given the initial and final ph. how do you determine how much of a strong acid...
given the initial and final ph. how do you determine how much of a strong acid to add to water to obtain the final ph. given intial ph = 4 final ph = 7 volume of water = 10 liters concentration of strong acid (HCL)= 3 moles/L So how much HCl (in mL) do we have to add to water to obtain the final ph of 4
For each strong acid solutions, determine [H3O+],[OH−], and pH. 1. 0.18 M HCL 2. 2.7×10−2 M...
For each strong acid solutions, determine [H3O+],[OH−], and pH. 1. 0.18 M HCL 2. 2.7×10−2 M HNO3 3. a solution that is 5.8×10−2 M in HBr and 2.3×10−2 M in HNO3 4. a solution that is 0.700% HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)
Titration 1: weak acid (CH3COOH) w/ strong base (NaOH) Titration 2: strong acid (HCl) w/ strong...
Titration 1: weak acid (CH3COOH) w/ strong base (NaOH) Titration 2: strong acid (HCl) w/ strong base (NaOH) - Concerning the above two titrations, answering the following questions: 1.) Calculate the theoretical equivalence point in terms of NaOH added for each of the titrations. Assume the concentration of acid is 0.81 M and the concentration of base is 0.51 M. 2.) Which equation can be used to find the pH of a buffer? Calculate the pH of a buffer containing...
In a titration of a 100.0mL 1.00M HCl strong acid solution with 1.00M NaOH, what is...
In a titration of a 100.0mL 1.00M HCl strong acid solution with 1.00M NaOH, what is the pH of the solution after the addition of 138 mL of NaOH? (3 significant figures) **Remember to calculate the equivalence volume and think about in which region along the titration curve the volume of base falls, region 1, 2, 3, or 4**
Calculate the pH of each of the following strong acid solutions. a. 4.28×10−2 M HNO3. b....
Calculate the pH of each of the following strong acid solutions. a. 4.28×10−2 M HNO3. b. 0.260 g of HClO3 in 2.40 L of solution. c. 20.00 mL of 2.00 M HCl diluted to 0.490 L . d. A mixture formed by adding 57.0 mL of 1.5×10−2 M HCl to 170 mL of 1.0×10−2 M HI.
In a titration of a 100.0mL 1.00M HCl strong acid solution with 1.00M NaOH, what is...
In a titration of a 100.0mL 1.00M HCl strong acid solution with 1.00M NaOH, what is the pH of the solution after the addition of 139 mL of NaOH? (3 significant figures)
QUESTION 1 What is the pH of a 1.5x10-8 M solution of HCl? a. 6.97 b....
QUESTION 1 What is the pH of a 1.5x10-8 M solution of HCl? a. 6.97 b. 7.03 c. 7.82 d. 6.18 1 points    QUESTION 2 What is the pH when [HA-] = [A2-] for a weak diprotic acid? a. pH = pK1 b. pH cannot be determined without concentrations. c. pH = 7.00 d. pH = pK2 1 points    QUESTION 3 The formula for Malonic acid is HO2CCH2CO2H and it is a weak acid (K1 = 1.42x10-3 ,...
Calculate the pH of each of the following strong acid solutions. 1. 20.00 mL of 1.50...
Calculate the pH of each of the following strong acid solutions. 1. 20.00 mL of 1.50 M  HCl diluted to 0.480 L . Express the pH of the solution to three decimal places. 2. A mixture formed by adding 46.0 mL of 2.5×10−2M  HCl to 120 mL of 1.5×10−2M  HI. Express the pH of the solution to two decimal places.
1) What is the pH of a 1.5x10^-8 M solution of HCl? 2) What is the...
1) What is the pH of a 1.5x10^-8 M solution of HCl? 2) What is the pH when [HA-] = [A^2-] for a weak diprotic acid? 3) The formula for Malonic acid is HO2CCH2CO2H and it is a weak acid (K1 = 1.42x10^-3 , K2 = 2.01x10^-6). What is the pH of a 0.25M solution of HO2CCH2CO2Na? 4) Leucine is a diprotic amino acid (K1= 4.677 x 10^-3 , K2= 1.820 x 10^-10). Determine the pH if 11.0 mL of...
For each strong acid solutions, determine [H3O+],[OH−], and pH. (So, there should be three answers for...
For each strong acid solutions, determine [H3O+],[OH−], and pH. (So, there should be three answers for each question). 1. 0.22 M HCl 2. 1.8×10−2 M HNO3 3. a solution that is 6.1×10−2 M in HBr and 1.9×10−2 M in HNO3 4. a solution that is 0.755% HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)