the pH of a 0.1 M KNO3 solution

Q: 11

A: Step-1: Calculate the H+ Value [H+] [OH-] = 1 x 10-14 H+ = [1 x 10-14]/ [OH-] H+ = [1 x 10-14]/ [1 x…

Q: the pH of the solution given that Kw=2.93×10^−15 at

A: The pH of the solution given that Kw =2.93×10−15 at this temperature

Q: Q3/ If the following solutions: (NaOH 0.145N, 50ml). (HSO. 0.105N, 22ml) (HCI 0.095N.40ml). Are…

A: Given: 50 mL of 0.145 N NaOH 22 mL of 0.105 N HSO 40 mL of 0.095 N HCl

Q: The pH of a chemical solution is given by theformula pH = - log10 [H+ ] where [H+ ] is the…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: 6. 7 6. 10 11 12 13 Fill in the missing chemical formulae in the tables below. acid conjugate base…

A: According to Bronsted Lowry concept, acid is substance which donate hydrogen and  base is substance…

Q: Calculate the pH of a solution that is 0.0729 M LiC2H3O2 at 25°C.

A: LiC2H3O2 ( Lithium acetate) is the salt of a weak acid and strong base.   LiC2H3O2 → CH3COO- +…

Q: What is the pH of a 0.109 M solution of HI? Enter your answer in decimal format with two decimal…

A: Given : Concentration of HI = 0.109 M

Q: What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179…

A:

Q: All of the following are weak acids except O HCNO O HBr O HF O HNO, O HCN

A: An acid which dissociates completely or almost completely in water are strong acids.An acid that…

Q: A solution has a pOH of 6.50 at 50∘C. What is the pH of the solution given that Kw=6.22×10−15 at…

A: To determine pH of solution: First we have to calculate pKw,

Q: What is the pH of a 0.0556 M NH, (aq) solution at room temperature? The base ionization constant of…

A:

Q: The pH of a solution of household ammonia, a 0.950 M solution of NH3, is 11.612. Determine Kb for…

A: We know that, pH can be expressed as the negative logarithm of H+, i.e.            pH = - log[H+]…

Q: The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid. (a) You are…

A: The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid.  (a) You…

Q: Determine the pH of a solution with (H30*) = 5.08 × 10-6 M. Your answer should contain 3 decimal…

A: The given data is as follows: H3O+=5.08×10-6 M The pH of the solution = ? The pH of a solution can…

Q: Calculate the pH of a 0.40 M solution of HCIO given that Ka (HCIO) = 2.9x108 Give your answer to 2…

A: PH of HClO can be calculated as follows

Q: Calculate [H3O+] for a solution with a pH of 4.80.

A: We know that pH of solution = -log[H+] or…

Q: Calculate pH if [H3O+]=4.02x10^-3 and [H3O+]=8.99x10^-7

A: pH = -log[H3O+]

Q: The pHpH of a 1.00 MM solution of caffeine, a weak organic base, is 12.300. Calculate the KaKa of…

A: In this question,  we have to find the pH of solution by the use of Henderson hessalbalch equation,…

Q: Calculate the pH of a solution that is 0.0736 M KC2H3O2  at 25°C.

A:

Q: Calculate pH of [H+] concentrations of 5.42x10-6 M and 9.98x10-12 M.

A:

Q: (i) Define pH in words. The strong acid HCla has a pH value of 1, use the following equation HCL ->…

A: We have to define pH and find the concentration of H+ ion

Q: At 25 °C, a solution has a

A:

Q: The pH of a solution is (6.5x10^0). What is the [OH-]? Report your answer to 2 sig figs. Note: Your…

A: Given, pH of the solution = 6.5 × 100 = 6.5 Concentration of the OH- ion = [OH-] = ? The formula…

Q: Determine the pH of a solution with (H3O*] = 5.08 × 10-6 M. Your answer should contain 3 decimal…

A: pH =-log {H3O+}  Let solve the question

Q: A solution has a pOH of 7.1 at 10∘C. What is the pH of the solution given that Kw=2.93×10−15 at this…

A: Kw=2.93 x10-15pkw=-log 2.93x10-15     =15-log 2.93pkw=15-0.466=14.534pH+pOH=pkwpH=pkw-pOH…

Q: A food product sample is tested for its pH, and is found to have a value of 5.7. What is the [OH^-]…

A:

Q: Given that for water at 37 °C Kw = 2.4x10 1 what is the pH of a neutral aqueous solution at 37 °C?…

A: for water , Kw = [H+] [OH-]   pH of water depends on temperature.

Q: The pH of a solution of HCl in water is found to be 1.20. what volume of water would you add to 1.00…

A: HCl is a strong acid so it is completely dissociated in the solution.

Q: An aqueous solution at 25 °C has a pOH of 6.85, Calculate the pH. Round your answer to 2 decimal…

A: pH of the solution is the measure of Hydrogen ion concentration which determines the strength of…

Q: The concentration of H3O+ in a solution is measured to be 6.27 x 10-3 Report the pH of the solution…

A: The pH of a solution is calculated by using the following expression: pH = -log[H3O+] where [H3O+]…

Q: The pH for 1.0 × 10⁻³ M solution of cocaine, a weak base, is 9.70. Determine the value of Kb for…

A: Cocaine can be denoted as B. Concentration of OH- ions in cocaine can be determined as follows,

Q: A solution of sodium acetate 1NaCH3COO2 has a pH of 9.70. What is the molarity of the solution?

A: pH scale is used to measure the acidity or basicity of the solution. If the solution is acidic in…

Q: if the H3O+ ion concentration in an aqueous solution at 25 °c measured 4.61 * 10^-8 M, what is the…

A: Given : [H+] = 4.61 * 10^-8 M

Q: Can you please provide a much detailed computation for this question? from given, formula,…

A:

Q: What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179…

A: Given : Percent by mass of HCl = 36.0 % Density of solution = 1.179 g/mL Volume of HCl solution to…

Q: The pH of a 0.20-M solution of HF is 1.92. Determine Ka for HF from these data.

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: Milk has a pH of 6.5. Determine the pH, to the nearest tenth, of a liquid with one quarter the…

A: Answer :-  pH of liquid with one quarter the concentration of hydrogen ions as milk = 7.1…

Q: at a certain temperature, the pH of a neutral solution is 7.87. What is the value of Kw at that…

A: We have to calculate the Kw for neutral solution.

Q: A Moving to another question will save this response. Question 4 Calculate the pH of a 0.0927 M…

A: Given, Concentration of the pyridine solution (C) = 0.0927 M Kb for pyridine (C5H5N) = 1.7 × 10-9 pH…

Q: culate the pH of a solution that is 0.0853 M LiNO2 at 25

A: Given : Molarity of LiNO2 = 0.0853M

Q: Complete the data sheet below. DETERMINATION OF pH OF DIFFERENT SOLUTIONS For those who will be…

A:

Q: Calculate the percent ionization of 0.0070 M butanoic acid (Ka = 1.5 × 10¬³). Express Vour answer to…

A:

Q: 8. Calculate the pH of NaOH(aq) to the nearest hundredth.

A: Given data : Molarity of NaOH = 0.20 M

Q: What volume of a 15.0% by mass NaOH solution, which has a density of 1.116 g/mL, should be used to…

A: the answer is follows as:

Q: The pH of an aqueous solution at 25.0 °C is 12.36. What is the molarity of H + in this solution?

A: Given information,      The pH of an aqueous solution at 25.0 °C is 12.36

Q: 7- Determine [OH-], [H*], and the pH of each of the following solutions. а. 1.0 М КСІ b. 1.0 М…

A: pH - pH is defined as negative logarithm to the base 10 of H+ ion concentration. Mathematically, pH…

Q: Which of the following acids is weaker

A: In the oxyacids higher the oxidation number of central atom, more stronger is the acidic.  So, HClO3…

Q: Calculate the pH of the following solutions: a) 1.9x10 10 M LIOH b) 6.6x10 MHCIO4 c) 0.35x10 2 M KOH…

A: Interpretation- To determine the pH of given solutions - 1.9 ×10-10 M LiOH  6.6×10-5 M HCIO4…

Q: For a 0.15 M H3PO4(aq) solution, determine pH [H3PO4], [H2PO4-], [HPO42-], and [PO43-]

A: Given: Concentration of H3PO4 = 0.15 M Ka1 = 7.1×10-3 Ka2 = 6.3×10-8 Ka3 = 4.5×10-13

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.