A 1.0M HCI solution has a volume of 20.0 mL. Determine the pH of the solution that results from adding each of the following: (assume addition of liquid volumes is additive, while addition of solids has no effect on volume) a. 5.0 mL of 1.0 M NAOH

Q: percent ionisation of the niacin.

A: To calculate the percent ionisation of the niacin we first calculate the [H+] pH = 3.26  [H+] =…

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Q: if 3,11•10^-4 moles of NaOH is reacted with 5,71•10^-4 moles of HCL,what is the pH if the total…

A: Consider the neutralization reaction between NaOH and HCl is as follows: NaOH + HCl → NaCl + H2O…

Q: A chemist dissolves 132. mg of pure hydrochloric acid in enough water to make up 60. mL of solution.…

A:

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: A chemist dissolves 721. mg of pure hydroiodic acid in enough water to make up 110. mL of solution.…

A: 1mole of HCl = 36.5 gr HCl is strong acid  so completely dissociate in water  HCl(aq) + H20…

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A: Weak electrolytes are those which do not dissociate completely rather there occurs equilibrium…

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A: phenolphthalein is a type of internal indicator . It is used as an indicator in acid base titration,…

Q: What is the pH of a solution if 10 mL of 1.0 M HCl is added to 10 mL of 3.0 M NaOH solution?

A:

Q: A solution is prepared by adding 49.7 mL concentrated hydrochloric acid and 19.1 mL concentrated…

A: Given: The volume of concentrated hydrochloric acid (HCl) is 49.7 mL The volume of concentrated…

Q: A solution is made by dissolving 36.7 g of HCl in 885 mL of water. Calculate the pH of the solution.

A: Given data of the following, mass of HCl = 36.7 g molar mass of HCl =36.458 g mol-1 Volume=885 ml =…

Q: A chemist dissolves 656. mg of pure barium hydroxide in enough water to make up 90. mL of solution.…

A:

Q: A solution contains 0.420 M CH3NH3 and 0.143 M methylamine, CH3NH2. The pH of this solution is .

A: Given : Concentration of CH3NH3+ = 0.420 M And concentration of CH3NH2 = 0.143 M Since the solution…

Q: The pH of an aqueous solution at 25°C was found to be 8.50. The pOH of this solution is The…

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M HCI with 40.00 mL of 0.10 M KOH?…

A: It is an example of acid base neutralisation reaction in which an acid is neutralises by the base…

Q: calculate how many millimeters of 1 M NaOH are necessary to make a 100.00 mL solution with a pH of…

A: Calculation  of millimeters  of 1M NaoH required  By dilution  law

Q: When answering this problem, report the answer with the appropriate number of significant figures.…

A:

Q: The pH of an aqueous solution at 25°C was found to be 3.80. The pOH of this solution is . The…

A: Given information, pH of aqueous solution at 25°C = 3.80 Formula used :  pH + pOH = 14 pH = -log…

Q: Two drops (0.1 mL) of 7.0 M HCl are added to water to make 1.0 L of solution. What is the pH of this…

A: Given: Concentration of HCl initially = 7.0 M Volume of initial HCl taken = 0.1 mL = 0.0001 L…

Q: How is calculating pH of a salt different than a calculating pH of a weak acid or base ?

A: An acid is a substance that gives  ions in its solution whereas a basic substance gives  ions in its…

Q: The pH of an aqueous solution at 25°C was found to be 12.00. The pOH of this solution is . The…

A: Given: The pH of an aqueous solution at 25°C was found to be 12.00. To find : The pOH of this…

Q: What is the concentration of hydroxide ion in a 0.160 M  aqueous solution of hydroxylamine, ? What…

A: Given: The concentration of the aqueous solution of hydroxylamine (NH2OH) is 0.160 M The Kb value is…

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A:

Q: When 90 mL of water is added to 10 mL of 0.1 M sodium hydroxide, NAOH, the pH.. .... O changes to 3.…

A: The pH of solution will before adding water : If [NaOH] = 0.1 M [OH-] = 0.1 M [H+][OH-] = 10-14 [H+]…

Q: The pH of an aqueous solution at 25°C was found to be 9.20. The pOH of this solution is The…

A: pH + pOH = 14  pOH = 14 - 9.2 = 4.8

Q: Determine the pH of a solution that is 1.55% NaOH by mass. Assume that the solution has density of…

A: pH: It is a scale that is used to get the idea of the acidity and basicity of an aqueous solution.…

Q: A solution contains 2.25 M acetic acid, 1.21 M sodium bromide, 0.85 M lithium bromide, and 0.80 M…

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Q: The pH of an aqueous solution at 25°C was found to be 3.40. ail The pOH of this solution is The…

A: The pH of the solution is equal to the negative logarithm of hydronium ion while pOH is equal to the…

Q: Determine the pH of an HF solution of each of the following concentrations. In which cases can you…

A: (a)ICE table for the reaction is given below.

Q: A 1.0m HCl solution has a volume of 20.0 mL. Determine the pH of the solution that results from…

A: For reactions containing base and acids, the pH depends on species containing lesser moles. If base…

Q: As much as 8 grams of NaOH (Mr = 40) is dissolved in water until the volume of the solution becomes…

A:

Q: 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…

A: Given volume of HCl = 50 mL = 0.050 L  As, 1000 mL = 1.0 L  Molarity of HCl = 0.3 M = 0.3 mol/L…

Q: what is the pH of a solution that is 1.05% HCl by mass (Assume a density of 1.01 g/mL for the…

A: Given information: Density is 1.01 g/mL 1.05% HCl

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Q: Calculate the pH of a solution when3.78grams of HCl was placed in 150.25 mL of water. HCl is a…

A: Solution -

Q: A chemist dissolves 227. mg of pure hydrobromic acid in enough water to make up 90. mL of solution.…

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

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

A: First we would Calculate pH of buffer solution using Henderson Hasselbalch equation.  When HCl is…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.9×10² M. The hydronium ion…

A: • The values provided in the question are:-    i) Hydroxide ion concentration of a solution, [OH-] =…

Q: A chemist dissolves 326. mg of pure potassium hydroxide in enough water to make up 130. mlL of…

A: Given: Mass of KOH = 326 mg = 0.326 g                                     (since 1 g = 1000 mg) And…

Q: solution is 3.75. what is the percent ionization for

A: Concentration of Acid(C) = 0.012 M pH = 3.75 pH = -log([H+)] = 3.75 [H+] = 10-3.75 = 0.000178 M

Q: Hydroiodic acid often is used to disinfect and sanitize medical tools and products. In an…

A: To predict pH without calculation we will observe the concentration of the HI acid before and after…

Q: A solution is prepared by adding 51.0 mL concentrated hydrochloric acid and 19.9 mL concentrated…

A: Given, Solution is prepared by adding: 51mL of 38% by Mass HCl solution 19.9 mL of 70% by mass HNO3…

Q: Enter your answer in the provided box. Calculate the pH of a 0.35 M KOH solution. pH

A: Given:   The molarity of KOH solution is 0.35 M.

Q: Suppose you have 557 mL of 0.0300 M HCI, and you want to make up a solution of HCl that has a pH of…

A: Since the pH = -log[H+]  And since HCl is strong acid hence it will dissociate completely  =>…

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.