To what total volume would you have to water down a 10ml 2.2M sample of HCl to get a final pH of 1.65?

To what total volume would you have to water down a 10ml 2.2M sample of HCl...
A 11.3-mL sample of an HCl solution has a pH of 2.085. What volume of water must be added to change the pH to 4.170? (in mL)
what volume of 0.25M HCl is needed to completely react with 10mL of 5M of NaOH?
1. 1x10^-9 moles of strong acid HCl are added to of water (total volume is 1L). the pH of the resulting solution is... a)9 b)8 c)7 d)5 e)2 I got 9 but got the answer incorrect, so i would like to know how to solve this properly and what is the final answer. 2. the pKa of acetic acid is 4.76. if the pH=4.76 and the concentration of sodium acetate is 0.1M, what is the concentration of acetic acid? a)0.05...
Zn + HCl ---> ZnCl2 + H2(g) The total volume of collected gas over water at 65oC was 1728 ml at a total pressure of 845 torr. If you used 325 ml of HCl for the reaction, what molarity of HCl would be required to produce the correct amount of Hydrogen?
If I have an initial concentration of NaOH of 1.25M in 15mL, and add 10mL water to get a final concentration of 25mL, what's the final concentration of the NaOH? I did C1V1 = C2V2 and got 0.5M Is that correct?
You need to load 2mg total protein in 10ml (i.e. final protein concentration needed is 0.2mg/ml for all the samples). You need to prepare 20 ml of this solution that has protein and 1X sample buffer (water is used for dilution). Complete the table below. Sample Protein Concentration mg/mL Protein Sample (microliter) Water (microliter) 4X Sample Buffer (microliter) Total Sample Volume (microliter) Total Lysate (-) 1 mg/mL 20 E1 0.07 mg/mL 20 E2 0.15 mg/mL 20 E3 0.2 mg/mL 20
9. What volume of 3.0 M HCl would need to be diluted with water to form 175 mL of 0.50 M HCl? (2)
you ask your lab partner to add 1mL to a 10mL water sample to 99 mL of diluent. Your partner inadvertently adds the entire sample of water to the diluent bottle. What was the intended dilution factor and what is the actual dilution factor?
A 50.0 mL sample of 0.436 M NH_4NO_3 is diluted with water to a total volume of 250.6 mL. What is the ammonium nitrate concentration in the resulting solution? 8.72 times 10^-2 M 21.8 M 0.459 M 0.109 M 2.18 times 10^-2 M If 24.95 mL of a 0.1025M HCL solution is added to reach the endpoint of a titration, how many moles of HCl have been added?
Concentrated hydrochloric acid (HCl) (molecular mass 36.5 g/mol) has a molarity of 3.6M. What volume of concentrated HCl would you need to add to prepare a 20% (w/v) solution of HCl with a final volume of 500 mL, I have calcualted that 3.6mol/L x 36.5g/mol =131.40g/L. Then to get the 100ml value and percentage: 131.40/1000 x 100 =13.14g/100ml therefore 13.14%. 20% of this would be 2.628g. Is this the answer?