What is the pH of a buffer solution made by adding 0.010 mole of solid NaF to 50. mL of 0.40 M HF? Assume no change in volume. Ka (HF) = 6.9x10 Item equation/constant pH = pK,+log| [A] %3D [HA] O 1.6 O 1.9 O 2.9 O 3.2

What is the pH of a buffer solution made by adding 0.010 mole of solid NaF to 50. mL of 0.40 M HF? Assume no change in volume. Ka (HF) = 6.9x10 Item equation/constant pH = pK,+log| [A] %3D [HA] O 1.6 O 1.9 O 2.9 O 3.2

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A buffer solution is made that is 0.498 M in HNO2 and 0.498 M in KNO2. If Ka for HNO2 is 4.50 x…

Q: A buffer solution is made that is 0.417 M in HC1O and 0.417 M in KC10. If K, for HC1O is 3.50 ×…

Q: A 50.0 mL sample of 0.100 M NH, is titrated with 0.100 M HBr. What is the most likely pH of the…

A: Answer :- 2.041 pH = 2.041…

Q: An industrial chemist studying bleaching and sterilizing pre-pares several hypochlorite buffers.…

A: Handerson Hasselbalch equation – Buffer solution is mixture of weak acid and its conjugate base.…

Q: A buffer solution is made that is 0.456 M in HC10 and 0.456 M in KC1O. If Ka for HC10 is 3.50 ×…

A: The Ka for HClO = 3.50×10-8 We have to calculate the pH of a buffer solution that is 0.456 M in HClO…

Q: What is the pH of the buffer solution that contains 2.0 g of NH4Cl in 250 mL of 0.050 M NH3? Is the…

A: Buffer solutions are designated as alkaline buffer solutions and acidic buffer solutions. Given…

Q: A buffer solution is made that is 0.357 M in HCN and 0.357 M in KCN. If K, for HCN is 4.00 × 10-10,…

Q: If Kal for H2 CO3 is 4.20 x 10-, what is the pH of the buffer solution? pH = Write the net ionic…

Q: A buffer is made up of 2.0 mL of 0.1 M weak acid (AH) and 20.0 mL of 0.1 M conjugate base (A minus).…

A: Given Volume of weak acid = 2 mL = 2 × 10-3 Liter ( 1 mL…

Q: A solution contains 0.24 M Pb²+ and 0.40 M Al³+. Calculate the pH range that would allow Al(OH)3 to…

A: Concentration of = Concentration of = of = of =

Q: A buffer solution is made that is 0.450 M in HF and 0.450 M in NaF. If Ka for HF is 7.20 × 10¬4,…

Q: A1 liter solution contains 0.467 M hydrofluoric acid and 0.350 M potassium fluoride. Addition of…

A: A weak acid partially dissociates in aqueous solution to form certain amount of conjugate base and…

Q: 57. The pH of normal, unpolluted rainwater is controlled by carbonic acid equilibrium: CO₂(g) →…

A: We have find out the answer.

Q: A buffer solution is made that is 0.481 M in HCIO and 0.481 M in NaCIO. If K, for HCIO is 3.50 x…

Q: A chemistry graduate student is given 500. mL of a 0.60M nitrous acid (HNO,) solution. Nitrous acid…

Q: You have 500 mL of a buffer solution conatining 0.154 M acetic acid (CH3COOH) and 0.158 M sodium…

A: we have to calculate the pH after NaOH is added to the buffer solution

Q: A 1.0-L buffer solution contains 0.100 mol acid, HA, and 0.100 mol base, NaA. The value of Ka for…

A: # We can calculate the pH of the solution using handerson-hasselbalch equation. # Added acid will…

Q: A buffer solution is made that is 0.406 M in HNO2 and 0.406 M in NaNO2. -4 If Ka for HNO2 is 4.50 ×…

Q: A buffer is prepared such that [CH3COOH], = [CH3C00-lo = 0.050 M. Calculate the volume of 0.10 M…

A: Millimoles of Acetic acid = M x V = 0.050 x 100.0 = 5.0 mmol = Millimoles of sodium acetate Let…

Q: A buffer solution is made that is 0.395 M in HCIO and 0.395 M in NaCIO. ces to access important…

A: Given Concentration of HClO,[HClO] = [Acid] =0.395 M Concentration of NaClO, [NaClO] = [Base] =…

Q: 1.0 L of acetate buffer is made by combining 0.50 M CH3COOH with 0.50 M CH3COONa. The Ka of CH3COOH…

Q: A 98-mL sample of 0.62 M HNO2 (Ka = 4.0 ´ 10–4) is titrated with 0.25 M NaOH. What is the pH of the…

A: Number of mmols = Molarity x volume (mL) Number of mmols of NaOH added = 0.25 x 30 = 7.5 mmol Number…

Q: Please don't provide hnad writtin solution.....

A: The concentration of Ag+ that remains is approximately 2.69 x 10-22 M.Explanation:Given that:Volume…

Q: A buffer solution is made that is 0.320 M in H2CO3 and 0.320 M in KHCO3. If Kal for H2 CO3 is 4.20 ×…

A: Solution: pH of acidic buffer = pka + log(KHCO3/H2CO3) pka1 of H2CO3 = -logka1 =…

Q: A buffer solution is made that is 0.450 M in HF and 0.450 M in NaF. If Ka for HF is 7.20 × 10-4,…

Q: What is the pH for a buffer made of 0.214 MNH 3 and 0.107 MNH 4 Cl ? K b for NH 3 is 1.8 * 10 ^ - 5…

A: Given data is as follows: The concentration of NH3 = 0.214 M The concentration of NH4Cl = 0.107 M…

Q: A buffer solution is made that is 0.386 M in HNO2 and 0.386 M in KNO2. If Ka for HNO2 is 4.50 ×…

A: Interpretation - The pH of the buffer solution and net ionic equation for the reaction that occurs…

Q: Calculate the pH of a 0.350 M solution of potassium phenolate, KC6H5O. Ka for phenol (CH5OH) is 1.0…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: IS IS If Kal for H2S is 1.00 x 10, what is the pH of the buffer solution? pH = Write the net ionic…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: A buffer is prepared by mixing 0.15 M NazHPO4 and 0.10 M NaH, PO4. K, for H3PO4 = 7.5 103 %3D Ka for…

A: The PH of buffer can be calculated as

Q: A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate.…

A: Given: Concentration of acetic acid i.e. CH3COOH = 0.200 M Concentration of sodium acetate i.e.…

Q: The p?apKa of hypochlorous acid is 7.5307.530. A 56.056.0 mL solution of 0.1000.100 M sodium…

Q: A chemistry graduate student is given 100. mL of a 0.30M diethylamine ((C,H;), NH) solution.…

Q: What volume in mL of 0.2572 M NaOH must be added to 500.0 mL of 0.1000 M chlorous acid (HClO2, Ka =…

A: Given: pH = 2.25 Concentration of HClO2 = 0.100 M Volume of HClO2 = 500.00 mL Concentration of NaOH…

Q: A chemistry graduate student is given 300. mL of a 1.10M benzoic acid (HCH,CO₂) solution. Benzoic…

Q: Which of the following molecules cannot exhibit intermolecular (among themselves) hydrogen bonding?…

Q: Complete the statement below regarding the pH of the solution at the equivalence point when 40.0 mL…

A: The analyte is 40.0 mL of 0.1 M propanoic acid (HC3H5O2). The titrants are NaOH and Ca(OH)2, both of…

Q: A buffer solution is made that is 0.402 M in HF and 0.402 M in KF. If Ka for HF is 7.20 x 10-4 what…

Q: Calculate the pH of a buffer that is 0.208 M lactic acid, HC3H5O3, and 0.208 M sodium lactate,…

A: Given that: Molarity of lactic acid = 0.208 M…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

What is the pH of a buffer solution made by adding 0.010 mole of solid NaF to 50. mL of 0.40 M HF? Assume no change in volume. Ka (HF) = 6.9x10 4
Item equation/constant:
pH = pK¸+log
[A]
[HA] )
O 1.6
O 1.9
O 2.9
O 3.2

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A buffer solution contains 0.53 mol of hydrosulfuric acid (H2S) and 0.10 mol of sodium hydrogen sulfide (NaHS) in 8.70 L.The Ka of hydrosulfuric acid (H2S) is Ka = 9.5e-08.(a) What is the pH of this buffer?pH = ____(b) What is the pH of the buffer after the addition of 0.44 mol of NaOH? (assume no volume change)pH = ____(c) What is the pH of the original buffer after the addition of 0.02 mol of HI? (assume no volume change)pH = ____
A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600M sodium acetate. What is the pH of a solution that results when 3.00 mL of 0.034 M HCI is added to 0.200 L of the original buffer? Use 1.80 x 10-5 as Ka for acetic acid and formula, pH = pKa + log [base]/[acid] %3D О3.46 5.22 4.86 3.86
7
A buffer solution is made that is 0.452 M in HC10 and 0.452 M in KC10. If K, for HC10 is 3.50 x 10-8, what is the pH of the buffer solution? pH : Write the net ionic equation for the reaction that occurs when 0.100 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +
Calculate the final [Ag1+] concentration in solution when 0.035 moles of AgNO3 are added to 500. mL of 0.21 M NaCN. Assume the volume remains constant. Ksp = 1.2 ✕ 10-16 for AgCN. (in M)
A buffer is made up of equal volumes of 0.1 M weak acid (AH) and 0.1 M conjugate base (A minus). The pH of the solution is measured to be 4.6. What is the pk, of this weak acid? (HINT: Use the formula pH = pK, + log(Vol A minus/ Vol HA)) %3D O 2.6 O 1.6 O 5.6 O 3.6 O 4.6
Calculate the pH of a buffer when 0.010 moles of NaOH is added to 100. mL solution that is 0.20 M sodium pentanoate (C HCOONa) and 0.20 M pentanoic acid (CH₂COOH). PK (CH₂ a COOH) = 4.82.