Question

Chemistry Question Part a) A solution of hydrofluoric acid contains 48.0% HF by mass and has...

Chemistry Question

Part a)

A solution of hydrofluoric acid contains 48.0% HF by mass and has a density of 1.15 g/mL at 25 °C. What volume of this solution should be used in a reaction requiring 1.25 mol HF? (Be sure to indicate the appropriate number of significant figures in the final answer.)

Part b)

What volume of 1.25 M HF(aq) must be diluted with water to prepare 0.500 L of 0.1 M HF(aq)? ​

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
Consider titration of 45.00 mL of 0.05982 M hydrofluoric acid, HF, with a standard 0.08780 M...
Consider titration of 45.00 mL of 0.05982 M hydrofluoric acid, HF, with a standard 0.08780 M solution of potassium hydroxide, KOH. The volume of the KOH solution needed to reach the equivalence point of the titration is ___________ mL. (Fill in the blank. Report the number only, with correct number of significant figures.) The pH at the equivalence point is ___________. (Fill in the blank, using the terms 7, > 7 or < 7 only.)
a. A 250.0 mL buffer solution contains 0.157 M RbF and 0.165 M HF. For HF,...
a. A 250.0 mL buffer solution contains 0.157 M RbF and 0.165 M HF. For HF, Ka= 3.5x10^-4 Label each as a strong or weak acid ;strong or weak base; acidic, basic or neutral salt: HF= _________RbF= ________ HBr= ___________ b. Write the hydrolysis reaction for HF (aq). c. Can the Henderson Hasselbach equation be used to calculate the pH? Why or why not? d. Calculate the pH of the buffer solution from part a. Show work! e. Write the...
Part A Calculate the mass percent (m/m) of a solution prepared by dissolving 52.18 g of...
Part A Calculate the mass percent (m/m) of a solution prepared by dissolving 52.18 g of NaCl in 152.8 g of H2O. Express your answer to four significant figures. Part B Vinegar is a solution of acetic acid in water. If a 185 mL bottle of distilled vinegar contains 26.5 mL of acetic acid, what is the volume percent (v/v) of the solution? Express your answer to three significant figures. Part C Calculate the mass/volume percent (m/v) of 24.0 g...
a solution that is made by combining 55 mL of 6.0×10−2 M hydrofluoric acid with 125...
a solution that is made by combining 55 mL of 6.0×10−2 M hydrofluoric acid with 125 mL of 0.12 M sodium fluoride I kept getting around 7.7 for the pH. I found the ml of HF and NaF to be (3.3*10^-3 mol) and (1.5*10^-2) respectively. The total volume to be 0.180L. and pKa value of 3.17 with a Ka value of (6.8*10^-4). The answer given was pH = 3.83 but I can't seem to get the same answer.
A solution of 500.0 mL of 0.500 M strong acid HA was used as part of...
A solution of 500.0 mL of 0.500 M strong acid HA was used as part of an electrolytic cell. The reduction half-reaction that took place was: 2 H+(aq) + 2e --> H2 (g) The hydrogen gas collected in this reaction occupied a volume of 98.00 mL at 22.0 oC and 738.5mm Hg. 1. How many moles of hydrogen gas were produced? ________ mol H2 2. How many moles of H+ ions were reduced? ________ mol H+ 3. What was the...
Background info: Vinegar contains acetic acid, CH3COOH. You can determine the mass of acetic acid in...
Background info: Vinegar contains acetic acid, CH3COOH. You can determine the mass of acetic acid in a vinegar sample by titrating with sodium hydroxide of known concentration. The reaction: CH3OOH(AQ) +NaOH(aq)=> CH3COONa(aq)+H2O(l). I have determined the grams of acetic acid to be 60. There are 25 ml sample of vinegar requiring 41.33 mL of a .953 M solution of NaOH by titrating sodium hydroxide of known concentration. ** THE QUESTION IS: What is the molar concentration of the acetic acid...
1.) An aqueous solution contains 0.23 M hydrofluoric acid. One Liter of this solution could be...
1.) An aqueous solution contains 0.23 M hydrofluoric acid. One Liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.12 mol HClO4 0.23 mol KNO3 0.24 mol HClO4 0.24 mol KF 0.117 mol NaOH 2.) An aqueous solution contains 0.34 M ammonia. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as...
A chemistry graduate student is given 250. mL of a 1.70 M chlorous acid (HClO2) solution....
A chemistry graduate student is given 250. mL of a 1.70 M chlorous acid (HClO2) solution. Chlorous acid is a weak acid with Ka = 1.1*10^-2. What mass of NaClO2 should the student dissolve in the HClO2 solution to turn it into a buffer with a pH = 1.89? You may assume that the volume of the solution doesn’t change when the NaClO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2...
A chemistry graduate student is given 450.mL of a 0.90M acetic acid HCH3CO2 solution. Acetic acid...
A chemistry graduate student is given 450.mL of a 0.90M acetic acid HCH3CO2 solution. Acetic acid is a weak acid with Ka=1.8x10^−5. What mass of KCH3CO2 should the student dissolve in the HCH3CO2 solution to turn it into a buffer with pH =4.35? You may assume that the volume of the solution doesn't change when the KCH3CO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
Part A: A calorimeter contains 32.0 mL of water at 12.5 ∘C . When 1.80 g...
Part A: A calorimeter contains 32.0 mL of water at 12.5 ∘C . When 1.80 g of X (a substance with a molar mass of 72.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 27.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water...