Calculate the pH of a solution which results from the mixing of 50 ml of 0.3 M HCI with 50 ml of 0.4 M NH3?

Q: A solution is prepared by adding 300 mL of 0.500 M NH3 and 100 mL of 0.500 M HCl. Assuming that the…

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Q: What is the pH of a solution when a) 19.0 ml of 0.100 M NaOH has been added to 20.0 ml of 0.100M…

A: To determine PH of solution a) given 19ml of 0.100M NaOH added to 20ml of 0.100M HCl b) 21ml of…

Q: When 0.20 mol of NaOH is added to 0.50 mol of weak acid HX, in a total volume of 1.00 L, the pH of…

A: This acid - base reaction between NaOH and weak acid HX form a buffer solution. So we will use…

Q: A 0.0015 M solution of a weak base has a pH of 9.84. Calculate Kb

A: We have given that pH of Weak base = 9.84 Concentration of Weak base = 0.0015M pH + pOH = 14 pOH =…

Q: Calculate the pH of 0.085 0 M pyridinium bromide, C5H5NH1Br2. Find the concentrations of pyridine…

A: Given information: Concentration of pyridinium bromide = 0.0850 M

Q: Calculate the [OH-] and pH of a mixture formed by adding 50.0 mL of 0.0.20 M HCl to 150 mL of 0.010…

A: Given : Concentration of HCl = 0.020 M                                                     (Assuming…

Q: Calculate pH for a solution that contains proton [H+] of 0.02 mM (milimole/L).

A: Given: The concentration of proton [H+] is 0.02 mM

Q: . Compute the pH and percentage of ionization for Given Kb for NH4OH is 1.8 x 10-5 0.1M NH4OH.

A: Given :

Q: For 280.0 mL of pure water, calculate the initial pH and the final pH after adding 0.024 mol of NaOH

A: pure water : pH = 7.00 moles NaOH = 0.024 [OH-]= 0.024 mol/ 0.280 L=0.0857 M pOH = - log 0.0857=…

Q: A) What is the PH of a solution in which 15 mL of 0.01 M NaOH has been added to 25 mL of 0.1 M HCI?

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Q: Calculate how many mililiters of 1 M HCl are necessary to make a 100.00 mL solution with a pH of…

A: We have 1M HCl solution, we have to calculate the volume of this solution needed to make 100 mL…

Q: A hydrochloric acid solution was prepared from a 200 ml mixture of [HCl] 0.0500 mol L-1 in 300 mL of…

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Q: Determine the pH of each solution. a. 0.10 M NH4CI c. 0.10 M NaCI b. 0.10 M NAC2H3O2

A: The pH of a salt of weak base and strong acid is given by, pH=12(-log Kw-log C+ log Kb) where Kw is…

Q: Butyric acid, C3H,COOH, has ionization constant of 1.54 x 105. a) Calculate the pH of 50.0 mL of a…

A: part C pH of the resulting solution can be calculated using the values of volume and molarity of the…

Q: Enter your answer in the provided box. The K, for benzoic acid is 6.5 x 10. Calculate the pH of a…

A: Given that : Ka for benzoic acid = 6.5 x 10-5 Concentration of benzoic acid = 0.13 M We have to…

Q: Two aqueous solutions are mixed: 50 mL of 0.150 M H2SO4 and 50 mL of 0.0385 M NaOH. What is the pH…

A: first to calculate the moles of each. H2SO4 releases 2 moles of H+ NaOH releases 1 mol of OH-   then…

Q: 4- A liter of solution contains 0.25 M HCOOH and 0.3 M HCOONA, calculate the pH of this solution.…

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Q: Calculate the pH of a mixture that contains 0.10 M of HNO3 and 0.23 M of HBrO.

A: Given solution is a mixture of two acids namely HNO3 and HBrO.

Q: What is the pH of a solution of 0.100M HCN mixed with 0.150M NaCN?  Assume the total volume is 1.00L

A: Using the formula for pH to calculate.

Q: What is the pH of a solution of HCL in which (HCI] = 2.6 x 10 M7 (2 decimals only)

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Q: Calculate the PH of a solution made by mixing equal volumes of 0.01M butanoic acid and 0.1M sodium…

A: Given the solution which is 0.1 M sodium butanoate and   0.01 M butanoic acid,this is an acidic…

Q: The pH of a 0.2 M solution of a weak acid HA is found to be 3.6. Calculate the Kb for A-

A: Wr will ionize HA , then calculate concentrations at equilibrium to find Kb .

Q: Enter your answer in the provided box. The K, for benzoic acid is 6.5 X 10. Calculate the pH of a…

A: Given- Ka for benzoic acid =6.5×105  Concentration of benzoi acid= 0.13M

Q: Calculate the pH of a solution when 10.00 mL of 0.1000 M NH3 is added to 20.00 mL of 0.1000 M HCl.

A: Given: Concentration of HCl = 0.100 M Volume of HCl solution = 20.00 mL = 0.020 L…

Q: of 45 > Assuming equal concentrations, arrange these solutions by pH. Highest pH HCN(aq) HI(aq)…

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Q: Butyric acid, C3H,COOH, has ionization constant of 1.54 x 10. a) Calculate the pH of 50.0 mL of a…

A: We have to predict the pH of acid and salt and pH upon mixing the solution.

Q: In the lab you have 500 ml of a 0.45 M Na2HPO4 stock solution. If you take 10 ml of the solution and…

A: pH is used to determine the concentration of hydronium ion.

Q: 1. Which is the pH of 1M NAOH solution? 2. Which is the pH of 1M HCI solution? 3. Which is the pH of…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Order the following three solutions from smallest to largest pH: (i) 0.030 M Ba(OH) 2  (ii) 0.040 M…

A: Given,  (i). 0.030 M Ba(OH)2 (ii). 0.040 M KOH (iii). pure water Order the following three solutions…

Q: A 30.0 mL aliquot of a solution is 0.25 M HCl . If 0.1 M NaOH is to be added to this solution,…

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Q: What is the pH of a solution containing 200ml of 0.01M acetic acid and 80ml of 2.5M sodium acetate

A: Interpretation -  To determine the pH of a solution containing 200mL of 0.01M acetic acid and 80mL…

Q: You add 15.00 mL of 0.700 M NaOH to 50.00 mL of pure water, and to this mixture you then add 5.00 mL…

A: Given: concentration of NaOH = 0.70 M volume of NaOH = 15.0 mL volume of water = 50.0 mL Volume of…

Q: 2. Calculate the pH of a solution when 10.00 mL of 0.1000 M NaOH is added to 20.00 mL of 0.1000 M…

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Q: What is the pH of a solution made by mixing 45.00mL of 0.1256M HCl with 20.00mL of 0.2006M NH3?

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Q: Calculate the pH of the resulting solution when 30.0 mL of 0.500M HBr is added to 25.00 mL of 1.00 M…

A: The reaction of HBr with NaNO2 can be shown by the balanced chemical equation as follows: HBr (aq)…

Q: Determine the pH of   (a) a 0.25 M NH3 solution.    (b) a solution that is 0.25 M NH3 and 0.40 M…

A: Ammonia is a weak base, it is a Lewis base.

Q: What is the pH of a solution of 0.100M HCN mixed with 0.150M NaCN?  Assume the total volume is…

A: Given data is as follows: The concentration of HCN solution = 0.100 M The concentration of NaCN…

Q: The ?a value for acetic acid, CH3COOH(aq)CH3COOH(aq), is 1.8×10−51.8×10−5. Calculate the pH of a…

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Q: You add 7.00 mL of 0.100 M NaOH to 50.00 mL of pure water, and to this mixture you then add 12.00 mL…

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Q: Order the following three solutions from smallest to largest pH:(i) 0.030 M Ba(OH)2 (ii) 0.040 M KOH…

A: EXPLANATION: pH is the measure of acidity or basicity of an aqueous solution.It is measure on the…

Q: Example: Calculate the pH of a solution prepared by mixing 2 mL of a strong acid solution (keep…

A: A numerical problem based on pH, which is to be accomplished.

Q: 1.What is the pH of a solution made by dissolving 1.2g lithium nitride to a total volume of 2.00L

A: Note: As per company policy we are supposed to attempt first question only. Please repost other…

Q: What is the pH of a solution that is 0.150 M in acetic acid (aka=1.8 x 10^-5)? What is the percent…

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Q: Calculate the pH of the following: 5) A solution that contains 0.10 M ammonium hydrochloride and…

A: In this solution we have a strong acid HCl which dissociate completely .  And another is a weak acid…

Q: 4. 4.00 g KOH was added to the less basic solution in number 3. What will be the resulting pH of the…

A: Given, Mass of NaOH = 5.00 g  Mass of Ba(OH)2 = 5.00 g  Gram molar mass of NaOH = 40 g/mol  Gram…

Q: Q2// 1000 ml of o.1M hydrochloric acid were added to 1000 ml of o.1M ammonium hydroxide, ammonium…

A: When the salt of strong acid is weak base is formed, pH is calculated using the formula, pH=7-…

Q: Ka for HCN is 6.2 x 10-10. The pH of an aqueous solution of 0.10M of NaCN is?

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Q: Example : Calculate the pH of a solution obtained by mixing 10 mL of the strong acid HCl solution (…

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Q: hat ph and %ionization of 0.100M arsenic acid H2AsO4

A: The pH scale is used to rank solutions in terms of acidity or basicity (alkalinity). Since the scale…

Q: Twelve drops (0.6 mL) of 9.0 M HCl are added to water to make 1.0 L of solution. What is the pH of…

A: First of all, we calculate the hydrogen ion concentration of the diluted solution. Then we calculate…

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.