Answered: Determine the pH of a 1.30 M solution…

Science

Chemistry

Determine the pH of a 1.30 M solution of CH3COOK. Ka(CH3COOH) = 1.8×10-5 Express your answer to

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 76QAP: A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a...

See similar textbooks

Related questions

Q: Calculate [H2Asc], [HAsc-], [Asc2-], and the pH of 0.050 Mascorbic acid H2C6H6O6, H2Asc. (Ka1=…

A: We have given that Molarity of ascorbic acid = 0.050 M Ka1 = 1.0×10-5 Ka2 = 5 × 10-12

Q: A diprotic acid has ka1= 4.3×10^-6 and ka2= 5.5×10^-9. What will be the pH of a 0.77 M solution of…

A: In this question, we want to determine the pH of the Solution of the acid. You can see details…

Q: 9. What is the concentration of hydronium (H0)the pH is 1.25? Write your answer to 3 significant…

A: The product of concentration of hydronium ion and concentration of hydroxide ion is equal to the…

Q: Determine the pH of a. 0.23 M solution of NH4BR. Express your answer to 2 decimal places.

A: pH is a measure of acidity of the solution and it is equal to the negative logarithm of hydrogen ion…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

A: Bronsted- Lowery acid base theory: According to this theory acid is a proton donar and base is a…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

A: Conjugate acid contain one more hydrogen atom and one more positive charge than the base that formed…

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

Q: Determine the pH of a 0.01462 M HNO3 solution. Record your answer to 2 decimal places.

Q: What is the pH of a solution with a hydronium concentration shown below? Round answers to 2 decimal…

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

A: formula ka conjugate base formula kb HF 6.8 *10-4 F- 1.470 * 10-11 CH3NH3+ 2.27 * 19-11 CH3NH2…

Q: Q1 Complete the following table: [OH¯] pH [H,O*] Acidic, Basic, or Neutral? 2.0x10-6 9.8 3.5x10-3…

Q: find the pH of a KOH solution that is aqueous and 1x10-7M.

A: pH is defined as negative logarithm of hydrogen ions.

Q: Name: 1. Determine the pH and pOH (to two decimal places) for each: (a) Pure water at 50 °C (Kw =…

A: Water undergoes self ionisation in the following manner- 2 H2O ↔ H3O+ + OH- The equilibrium constant…

Q: Calculate the pH of a 0.0394 M solution of calcium hydroxide. Express your answer to the correct…

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What is the pH of a solution with a concentration of 2.20 × 10-5 M H+? Report your answer to two…

A: Given, The concentration of H+ = 2.20 x 10-5 M. pH is the negative logarithm of hydrogen ion…

Q: the [OH^-] was measured to be 5.60 x 10^-10 M then what is the pH

Q: 1) Determine the pH for each of the following (show your calculations; answer to two decimal…

Q: Determine the pH of a 0.031 M solution of Sr(OH)2. Enter your answer with four total significant…

Q: The kw for water is 5.5 x 10-14 at 50oC. What is the pH of a neutral aqueous solution at 50oC?…

Q: The pH scale 7 8 9 10 1II 12 13 14 +++++ 01 2 34 What do we call substances with pH of greater than…

A: Acid - Those species which give H+ ion on dissolving in water. Ph of acid is below 7 Base - Those…

Q: (a) pH is defined as the negative logarithm of hydrogen ions (H+), mathematically it can be…

A: pH is defined as the negative logarithm of [H^+]. Mathematically, pH = -log[H^+] =…

Q: An aqueous solution at 25.0°C contains [H+] = 0.099 M. What is the pH of the solution? Group of…

A: We have given that the concentration of [H+] = 0.099 M we know the formula to calculate the pH of…

Q: The pH of a 0.043 M solution of Sr(OH)2 is ________. Report your answer to two decimal places.

A: Strontium hydroxide is a strong base and it dissociated in the aqueous solution to give two…

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90x10–4 at 25°C. Calculate the pH of a 0.103 M solution of…

A: Initial concentration of (CH3)2NH = 0.103 M Kb = 5.90x10–4

Q: Calculate the pH of the acid or base with the given information. Given pH of 0.1 M ammonia…

Q: At 25.0 oC, Kw = 1.0 x 10-14 and neutral water has a pH of 7.00. At 98.4 oC, Kw = 5.11 x 10-13 and…

A: Kw = 5.11 × 10-13 Neutral water has a pH of .....?....

Q: Find the pH of a solution that is 5.0×10-2 M in H2CO3. Express your answer using two decimal places.…

Q: Kw of water at 100°C is 5.62 x 10-13. What is the pH of water at this temperature

A: Given- Kw = 5.62 × 10-13 T= 100°C = 100 + 273 = 373 K

Q: Determine the pH of a weak acid, HA, that has a concentration of 0.015 M and a Ka = 0.00005. Enter…

A: Given : Molarity of HA = 0.015M Ka = 0.00005

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

Q: propanoic acid, a weak monoprotic acid (HC3H5O2, Ka = 1.3 x 10-5), calculate [H+] and pH of a 0.10 M

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

Q: Determine the pH of a 1.58 x 10-6 M HI solution. Your answer should contain 3 decimal places as this…

Q: The Kb of (CH3)3N is 6.4x10^-5. What is the pH of a 0.48 M solution of (CH3)3NH+?

A: Given: The Kb of (CH3)3N = 6.4 × 10-5 We have to calculate the pH of a 0.48 M solution of (CH3)3NH+.…

Q: What is the final pH of a 2.86 M solution of arsenic acid, H3AsO4, where Ka1 = 5.5 x 10^-3, Ka2 =…

Q: The acidity or alkalinity of a solution is defined by pH = –log[H+] where [H+] is the hydrogen ion…

A: The pH of the apple juice can be determined as follows: pH = -logH+pH = -log3 × 10-4pH = 4 -…

Q: The pH scale 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 +++++ What do we call substances with a pH of 7?…

A: The pH scale is used for the detection of how acidic or basic is a substance. The pH scale ranges…

Q: The pH of 0.20 M HN03 is O a. 1.58 Ob. 0.70 C. 0.20 Od. 0.63

A: Using formula in these questions: PH = -log[H+] Where as [H+]-------> concentration of H+ Using…

Q: [H,0"]w1 Complete the table. That is, fill in any missing entries in the second and third columns.…

A: Given For solution A concentration of hydronium ion = 5.6 X 10-9 mol/L For solution C concentration…

Q: On campus lab students generally record a value of 7.5 for water with their pH meters. Offer 2…

A: pH is the measure of the amount or concentration of H+ ions present in the solution or how acidic or…

Q: The pH of a solution is given by the formula pH= -log [H^+], where [H^+] is the concentration of…

A: Applying concept of pH determination PH= - log[H+]

Q: Determine the pH of each of the following solutions. 0.19 M CH3NH3I(Kb(CH3NH2)=4.4×10^−4) Express…

A: Given 0.19 M CH3NH3I(Kb(CH3NH2)=4.4×10^−4) We have to Determine the pH of each of the following…

Q: What is the pH of (5.27x10^-1) M LİNO3? Enter your answer in scientific notation with 3 sig figs. Do…

Q: Complete the table. That is, fill in any missing entries in the second and third columns. Round your…

A: pH is defined as the negative logarithm of concentration of proton. pH=-log[H+] It tells about the…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

Q: Calculate the density of the unknown metal. Choose the answer with the correct number of significant…

A: "Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

A: According to the Bronsted-Lowry theory, an acid is a proton donor, and a base is a proton receptor.…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

100%

Determine the pH of a 1.30 M solution of CH₃COOK.
K_a(CH₃COOH) = 1.8×10^-5
Express your answer to 2 decimal places.

pH =

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

Calculate the pH of a 0.0058 M solution of ascorbic acid (a weak acid). Ka = 7.9×10-5 Express your answer to two decimal places. pH =
The pHpH scale for acidity is defined by pH=−log[H+]pH=-log[H+] where [H+][H+] is the concentration of hydrogen ions measured in moles per liter (mol/L). (A) If there are 0.0079432823472428 mol/L of hydrogen ions in a certain substance, what is the pH of this substance?pH=pH= Round your answer to at least two decimal places. (B) If there are 0.003019951720402 mol/L of hydrogen ions in a different substance, what is the pH of this substance?pH=pH= Round your answer to at least two decimal places.
6- Calculate the pH of a 8.0 x 10 ´M aqueous solution of hydrobromic acid (HBr). Round your answer to 2 decimal places.
Consider the following chemical equilibrium for the weak base CN in water: CN- (aq) + H₂O(1) = HCN (aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d pH will go up; [OH-] will go up; net amount of OH will go up pH will go down; [OH-]will go up; net amount of OH will go down pH will go down; [OH-]will go down; net amount of OH will go down pH will go up; [OH-] will go up; net amount of OH will go down
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H¹] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.171, the hydrogen ion concentration is mol/L.
Be sure to answer all parts. Determine the pH and percent ionization for a hydrocyanic acid (HCN) solution of concentration 6.2 x 103 M. (K, for HCN is 4.9 x 10 10.) pH = percent ionization = x 10 %3D (Enter your answer in scientific notation.)
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H+] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.735, the hydrogen ion concentration is mol/L.
ALEKS K O ACIDS AND BASES Calculating the pH of a dilute acid solution -9. Calculate the pH of a 7.5 x 10 M aqueous solution of hydrochloric acid (HC1). Round your answer to 2 decimal places.
Calculate the concentration of OH ions in a 3.20 × 10 M HCl solution. Round your answer to 3 significant digits. -3 Note: Reference the Fundamental constants table for additional information. [OH ]-M X10 X S
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = - log [H*] where [H"] is the hydrogen ion concentration. a If the hydrogen ion concentration in a solution is 1.97 x 10 molL, the pH is b. If the pH of a solution is 3.146, the hydrogen ion concentration is mol/L.
Suppose a 0.018M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibrium molarity of HPO4. You'll find information on the properties of phosphoric acid in the ALEKS Data resource. Round your answer to 2 significant digits. OM
Strong Acids; Calculate pH [HA]o [H;O"] pH Step 1 Calculate [H3O] based on the fact that strong acids react completely with water. Step 2 Calculate the pH using the equation: pH = -log (H;O"] What is the pH of a 1.73×10 M solution of the strong acid HC10,? HCIO,(aq) + H20(1) → C10, (aq) + H3o*(aq) [HC10], = 1.73×10-5 Submit