Benzoic acid (C6H5COOH) is a monoprotic weak acid with Ka = 6.30 x 105. What is the pH%3Dof a solution of benzoic acid that is 0.559M in benzoic acid and has 2.25 x 10?M NaOHadded?On aguenus selution is composed of acetic acid and sodium hydroxide. The acetic acid istho nH of the solution?

[Benzoic acid] = 0.559 M [NaOH] = 0.0225 M

Answered: Benzoic acid (C6H5COOH) is a monoprotic…

Benzoic acid (C6H5COOH) is a monoprotic weak acid with Ka = 6.30 x 105. What is the pH %3D of a solution of benzoic acid that is 0.559M in benzoic acid and has 2.25 x 10-2M NaOH added?

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 solution is prepared at 25 °C that is initially 0.11 M in dimethylamine ((CH,) NH), a weak base…

A: [(CH3)2NH] = 0.11 M [(CH3)2NH2Cl] = 0.44 M Kb = 5.4 × 10-4

Q: the solutions are additive and that Kp = 4.4 x 104 for methylamine.

A: The question is based on the concept of EQUILIBRIUM. we have to calculate pH of the solution…

Q: The base constant for ammonia, NH3, is Kb = 1.8 x 10-5. A solution was made up with ammonium…

Q: An analytical chemist is titrating 83.1 mL of a 0.2800M solution of piperidine (C5H10NH) with a…

A: According to the question we have the reaction for the piperidine (C5H10NH ) and iodic acid (HIO3):-…

Q: Calculate the pH of a solution containing 22 mL of 1.09 M of a weak weak base B OH, like NH4OH, or…

Q: Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the…

A: The dissociation of tartaric acid can be represented as: H2C4H4O6+H2O↔HC4H4O6-+H3O+…

Q: What is the pH of a solution that is 0.10 M in acetic acid, HC2H3O2, and 0.52 M in sodium acetate,…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: What is the pH of a solution prepared by combining 0.696 mol of a weak acid (Ka = 5.5 x 10-5) with…

A: we need to calculate pH of the solution

Q: What is the pH of the resulting solution if 45.00 mL of 0.10 M acetic acid is added to 10.00 mL of…

A: Given data contains, Volume of acetic acid is 45.00mL. Molarity of acetic acid is 0.10 M. Volume of…

Q: what is the pH of a solution prepared by mixing 15.0 mL of 0.50 M NaOH and 30.0 mL of 0.50 M benzoic…

A: The measurement of pH is widely used in various applications such as in agriculture, environmental…

Q: A 0.100 L solution is composed of 0.500 M (CH3)2NH and 0.500 M (CH3)2NH2Cl at 25 oC. What is the pH…

A: The objective of the question is to calculate the pH of the solution after the addition of .A buffer…

Q: HCN is a weak acid (K₁ = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…

Q: 3/3.5 6377 100 9. If a 50.0-mL sample of 0.250 M NaCN is titrated by 20.0-mL of 0.250 M HCI (strong…

A: To determine the pH of the solution resulting from the titration, we need to consider the reaction…

Q: A solution of acids is made by mixing 0.19 M HNO3 and 0.45 M CH3COOH (Ka (CH3COOH) = 1.8 x 10-5).…

A: To calculate the pH of the solution, we need to consider the acid dissociation reactions of both…

Q: What is the pH of a solution

Q: Calculate the pH of a solution that is 0.214 M acetic acid and 0.152 M sodium acetate. The Ka of…

Q: Without doing any calculations, which of the following acids, if in solutions of equal…

A: 11. Ka is the ratio of product of concentration of products raised to their stoichiometric…

Q: An aspirin tablet contains 250 mg of acetylsalicylic acid, C9H8O3 (Ka = 6.4x10-4). If you take the…

A: Answer :- pH = 2.30 pH of mixture of 250 mg acetylsalicylic acid, C9H8O4 in 35.0 mL water is 2.30…

Q: Name: NetID: 8. A titration is carried out where 50.0 mL of 0.300 M HF is titrated with a 0.190 M…

Q: A solution NH3 that contains 78 mL of 0.043 M ammonia, NH 3, is titrated with 0.083 M HCI. The K₁ of…

A: Given,Molarity of NH3 = 0.043 Mvolume of NH3 = 78 mLMolarity of HCl = 0.083 MKb of NH3 = 1.8 x 10-5

Q: pose 26.5 mL of 0.19 M NaOH is added to 45.3 mL of 0.24 M HCHO2. What will be the pH of the…

A: Molarity of HCOOH= 0.24 M Volume of HCOOH= 45.3 ml Molarity of NaOH = 0.19 M Volume of NaOH =…

Q: Calculate the pH of a solution that contains 3.25 M HCN (K a = 6.2 x 10 -10 ), 1.00 M NaOH and 1.50…

A: Detail

Q: The acid-dissociation constant (Ka) of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10. What is the…

A: NaCN → Na+ + CN- CN- + H2O ⇔ HCN + H3O+ The data given are- Ka of…

Q: What is the pH of a solution that is 0.28 M in acetic acid, HC2H3O2, and 0.69 M in sodium acetate,…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a solution…

Q: A solid hydroxide, with the formula M(OH)3, is dissolve to make a saturated solution. If the pH of…

A: Solubility indicates the maximum amount of a substance that can be dissolved in a solvent at a given…

Q: Calculate the pH of a buffer solution that is 0.120 M acetic acid and 0.110 M of the corresponding…

Q: A weak base, BOH, has a ph of 9.80 and Ka equal to 1.0 x 10-5. What is the Molarity of BOH?

A: Given data, The pOH of a weak base is calculated as shown below.

Q: 4-(N-Morpholino)butanesulfonic acid (MOBS) is a weak acid used to prepare buffers for biological…

A: Given,The mass of 4-(N-Morpholino)butanesulfonic acid (MOBS) = 5.00 g pKa of MOBS = 7.48 Molar mass…

Q: A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.14 M…

A: Given: Concentration of NaOH = 1.14 M Volume of HA solution used = 25.0 mL = 0.025 L…

Q: Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5. FW(propanoic acid) = 74.08 g/mol; FW(calcium…

A: Buffers are generally good over the range pH = pKa ± 1. For example, the acetate buffer would be…

Q: alculate the pH of a titration solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of…

A: Given 45.0 mL of 0.100 M NaOH is added to50.0 mL of 0.100 M CH3COOH (Ka = 1.8×10-5). pH is to be…

Q: HCN is a weak acid (K, = 6.20 × 10-0), so the salt, KCN, acts as a weak base. What is the pH of a…

A: Dear student I have given answer to your question in the image format.

Q: At a particular temperature, the Ka of benzoic acid (C6H5COOH) is equal to 7.1 x 10-5. What is the…

Q: What is the pH of 0.025 M aqueous acetate ion? (Kb of CH3C

A: According to Ostwald’s Dilution Law and the pH (& pOH) scales, we can derive pOH =…

Q: What is the pH of a buffer solution that is 0.21 M methylamine and 0.20 M methylammonium chloride?…

A: The solution can be easily determined using the Handerson HasselBach equation- pOH = pKb + log…

Q: What is the approximate pH at the equivalence point of a weak base-strong acid titration if 50.00 mL…

A: Molarity of HCl = 0.1087 mol/LpKb = 4.75

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

Benzoic acid (C6H5COOH) is a monoprotic weak acid with Ka = 6.30 x 105. What is the pH
%3D
of a solution of benzoic acid that is 0.559M in benzoic acid and has 2.25 x 10?M NaOH
added?
On aguenus selution is composed of acetic acid and sodium hydroxide. The acetic acid is
tho nH of the solution?

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

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

The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood is HCO, /H2CO3, A) determine the ratio [HCO,]/[H2CO3] in blood plasma. The ionization con- stant of carbonic acid is K.(H2CO3) = 4.3 x 10-7. B) Based on your result in part (A), how many moles of H2CO3 (assuming that they occupy no volume) would need to be added to 300.0 mL of an aqueous solution that is 0.250 mol L- in NaHCO3 to make a buffer solution of the same pH as blood plasma? To solve the problem you may assume that the solutions behave as ideal dilute solutions (solute-type activity coefficients equal to unity).
A solution contains 0.351 M HA (Ka = 1.13⋅10−51.13⋅10-5) and 0.744 M NaA. What is the pH of this solution? What is the pH of this solution after 0.186 mol of HCl are added to 1.00 L of this solution? What is the pH of this solution after 0.372 mol of HCl are added to 1.00 L of this solution?
HCIO is a weak acid (Ka = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a solution that is 0.039 M in NaCIO at 25 °C? pH =
Determine the pH during the titration of 59.5 mL of 0.490 M hypochlorous acid (Ką = 3.5×10-8) by 0.490 M NaOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.3 mL of NaOH
The ionization constant of acetic acid HC2H3O2 is 1.8 x 10-5. What will be the pH of a 0.10 M HC2H3O2 solution which is 0.10 M in NaC2H3O2
A solution is obtained by dissolution of 10-3 moles of phosphoric acid H3PO4 and 1.3×10−³ moles of NaOH in one litre of water. Calculate the pH of the mixture. The answer: pH = 6.8
The answer I got was 13.33 but that's not correct
what is the ph of 0.0349 M anilinium hydrochloride (C6H5NH3CI) solution in water, given that K for aniline is 3.83 x 10 -4
When 25.00 mL of 0.467 M NaOH was added to 50.00 mL of a 0.467 M solution of a weak acid, HX, the pH of the mixture reached a value of 3.49. What is the Ka of the weak acid? Ka=
Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M NH3. The Kb for NH3 is 1.8 × 10-5
HCN is a weak acid (K = 6.20 × 10-10), so the salt, KCN, acts as a weak base. What is the pH of a solution that is 0.0405 M in KCN at 25 °C? 10.40 pH = Incorrect