A 1.0 × 10 -2  M aqueous solution of Ca(OH) 2 at 25.0 °C has a pH of? 12.30     12.00     2.0 × 10-2      5.0 × 10-13      1.70

Q: Determine the pH of a solution that is prepared by dissolving 4.6 g of Ba(OH)2 in 3.3 L water at…

A: Number of moles (n) of solute present in 1 litre solution is called " Molairty (M) " M = n / V (in…

Q: Calculate the pH when 45.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 ×…

A: Molarity of HBr = 0.200 mol/LMolarity of CH3NH2 = 0.400 mol/LKb = 4.410-4Kw = 1.010-14

Q: Determine the pH of a solution that is prepared by dissolving 4.7 g of Ba(OH)2 in 5.6 L water at…

A:

Q: A chemist must prepare 450.0 mL of hydrochloric acid solution with a pH of 1.30 at 25 °C. He will do…

A: Volume of dil. HCl = 450.0 mLpH of dil. solution = 1.30molarity of conc. HCl = 9.0 M

Q: A solution is prepared at 25 °C that is initially 0.46 Min methylamine (CH₂NH₂), a weak base with K…

A:

Q: What is the equilibrium pH of an initially 0.37 M solution of a weak acid HA at 25°C? Ka = 4.89 x 10…

A: Acid dissociation constant Ka is utilized to determine the acidic and basic nature of a solution. It…

Q: Calculate the pH of a 4.80×10-1 M aqueous solution of sodium nitrite (NaNO2). (For nitrous acid,…

A:

Q: How many grams of NH4Cl (53.49 g/mol) must be dissolved in 0.639 L of solution in order to obtain a…

A: we need to find mass of NH4Cl in the solution for a pH 4.79

Q: For the diprotic weak acid H₂A, Kal What is the pH of a 0.0750 M solution of H₂ A? pH = = = 3.7 ×…

A: Given, The concentration of H2A = 0.0750 M. Ka1 = 3.7 × 10-6  and  Ka2 = 5.4 × 10-9 The pH of the…

Q: Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution…

A: Answer: Hydrolysis of the salt of weak acid and strong base or strong acid and weak base takes place…

Q: What is the pH of a solution of 0.79 M acid and 0.55 M of its conjugate base if the ionization…

A:

Q: Consider the following data on some weak acids and weak bases: acid Ka base name formula K, name…

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Q: Calculate the pH of a 0.563 M solution of NaF. The Ka for the weak acid HF is 6.8 x 10-4. pH =

A:

Q: 0.21 М CН3NH3І (Къ(СH3NH2) — 4.4 x 10-4)

A:

Q: A chemist must prepare 500.0 mL of hydrochloric acid solution with a pH of 1.20 at 25 °C. He will do…

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Q: Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution…

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Q: Phenol is a weak acid with a Ka = 1.28 x 10-10.  As a pure compound, it is rather corrosive but in…

A: Phenol (PhOH) will give the below reaction in water. PhOH ----> PhO- + H+ assuming a…

Q: The base protonation constant K of morpholine (C4H₂ONH) is 2.14 × 10 Calculate the pH of a 1.5 M…

A: Given,molarity of morpholine ( C4H8ONH ) = 1.5 MKb of morpholine ( C4H8ONH ) = 2.14 x 10-6

Q: A chemist must prepare 550.0 mL of nitric acid solution with a pH of 0.80 at 25 °C. He will do this…

A:

Q: An aqueous solution of 0.045 M HA (pKa = 11.11) is prepared. What is the pH of this solution? Enter…

A: The objective of this question is to calculate the pH of an aqueous solution of a weak acid HA with…

Q: What is the pH (to two decimal places) of a 0.15 M NH3 and 0.15 M ammonium chloride aqueous solution…

A: The pH of buffer can be calculated by using Handerson equation . Ammonia and ammonium chloride forms…

Q: Consider the following data on some weak acids and weak bases: acid base K, name formula hame…

A:

Q: A chemist must prepare 600.0 mL of hydrobromic acid solution with a pH of 1.90 at 25 °C. He will do…

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Q: A solution is prepared at 25 °C that is initially 0.44M in ammonia (NH3), a weak base with K₂= 1.8 ×…

A: Solution that  contains weak base (ammonia) and corresponding salt (ammonium chloride) of strong…

Q: at 95 ℃ water has an autoionization constant (Kw) of 4.518 X 10-13. Determine the ph of pure water…

A: Given :- Kw at 95°C = 4.518 × 10-13  To determine :- pH of pure water at 95°C

Q: Consider a 1.0-L solution that is initially 0.580 M NH3 and 0.780 M NH4Cl at 25 °C. What is the pH…

A: Given data:Calclate the pH of solution.

Q: A chemist must prepare 550.0 mL of nitric acid solution with a pH of 1.90 at 25 °C. He will do this…

A: Given that,  pH of 550 mL (V1) HNO3 solution at 25°C  = 1.90 Since, HNO3 is a strong acid and it…

Q: Calculate the pH and the equilibrium concentration of $² in a 5.45×10² M hydrosulfuric acid…

A:

Q: Consider the following data on some weak acids and weak bases: name acetic acid hydrocyanic acid…

A: The question is based on the concept of pH of the solution.  it is defined as a negative logarithm…

Q: 110 M in formic acid (K₂ = 1.8 × 10

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Q: Calculate the pH of a 0.30 M solution of HCN (weak acid). Ka for HCN is 4.9 x 10-10

A: Given: Concentration of the HCN solution = 0.30 M Ka for HCN = 4.9 × 10-10 We have to calculate the…

Q: Determine the pH of a solution that is prepared by dissolving 8.7 g of Ba(OH)2 in 2 L water at 25°C.…

A: Given: Mass of Ba(OH)2 dissolved = 8.7 g. And volume of solution = 2 L

Q: A triprotic acid (H3Y) has the following acid ionization constants: Ka1 = 5.3 x 104 Ka2 = 1.7 x 10-8…

A: Given: pH=6.93Ka1​=5.3x10−4;Ka2​=1.7x10−8;Ka3​=3.2x10−11Step 1: Solve for the pKa values of each…

Q: Determine the pH of a solution that is prepared by dissolving 7.9 g of Ba(OH)2 in 1.9 L water at…

A: Molar mass of Ba = 137.3g/mol  Molar mass of O = 16.00g/mol  Molar mass of H = 1.008g/mol

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A:

Q: An aqueous solution of 0.045 M HA (pKa = 11.11) is prepared. What is the pH of this solution? Enter…

A: The objective of this question is to calculate the pH of an aqueous solution of a weak acid HA with…

Q: chemist must prepare 200.0 mL of nitric acid solution with a pH of 1.20 at 25 °C. e will do this in…

A: Given that: The volume of nitric acid, V1 = 200 mL pH = 1.20 molarity of nitric acid, stock…

Q: Diisopropylamine, C6 H14NH, is a weak base. A 0.66 M aqueous solution of diisopropylamine has a pH…

A: We have to predict the Kb and the pH of Solution.

Q: Determine the pH of a solution that is prepared by dissolving 6.9 g of Ba(OH)2 in 4.5 L water at…

A:

Q: Consider the following reactions: SO32 (aq) + H2O(l) = HSO3(aq) + OH(aq) HSO3(aq) + H2O(l) =…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: A chemist must prepare 450.0 mL of nitric acid solution with a pH of 1.60 at 25 °C. He will do this…

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Q: Unit 2: Chemical Systems & Equilibrium Butanoic acid, C3H₂COOH, gives rancid butter its distinctive…

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Q: Assuming 0.1 M concentrations, arrange the following acid solutions in order of increasing pH.…

A: Concentration of each given acid = 0.1 M (c) We know that -> [H+] = √(Ka ×c)

Q: For a certain acid pK, = 7.13. Calculate the pH at which an aqueous solution of this acid would be…

A: The objective of the question is to calculate the pH at which an aqueous solution of an acid would…

Q: Calculate the pH of a 0.175 M solution of aqueous ammonia. Kb = 1.8 x 10-5

A: Write the equilibrium expression for the base dissociation of ammonia:NH3​+H2​O⇌NH4+​+OH− Write the…

Q: Consider a 0.015 M hypochlorous acid solution (Ka = 3.0 x 10-8). pH = a =

A: pH and α is calculated by dissociation of hypochlorous acid and using the value of Ka.

Q: A certain base has a Kb of 7.8 × 10-6 . What concentration of the base will produce a pH of 11.32?

A: Fristly we calculate the concentration of OH- from the pH : pOH = 14-pH  = 14-11.32 =2.68…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 x 10-4 and Ka2 = 6.7 x 10-⁹. What is the pH of a 0.64 M solution…

A:

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.