You have a 0.0685 M solution of Ca(OH)2, what is the pH of your solution?

Q: Calculate the pH of a solution in which [OH−]=7.1×10−3M.

A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…

Q: What is the pH of a 0.45 mol/L solution of hydrobromic acid? The answer should be to the proper…

A:

Q: 6) If the hydroxide ion concentration of a solution is 1.0 x 10° M Is it an acidic or basic…

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Q: Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the…

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Q: Calculate the pH of a 0.25 M solution of aluminum chloride, which dissolves completely to give the…

A: Concentration of aluminum chloride solution = 0.25 M   The equation for the reaction: Al(H2O)63+(aq)…

Q: You have a 1.25 L solution with 2.14 g of NaIO and the pH is 11,32. What is the Kb of NaIO?

A: Solution pH, pKa, pKb, Ka, and K ar employed in chemistry to explain however acidic or basic an…

Q: The pH of an aqueous solution of 0.134 M sodium fluoride, NaF (aq), is This solution is

A: Answer:- This question is answered by using the simple concept of calculation of pH of aqueous…

Q: Calculate the pOH and the pH of the following aqueous solutions at 25⁰C: (a)1.25 M LiOH (b) 0.22 M…

A:

Q: 2.00 L of sulfuric acid, H2 SO4 (ag), contains 0.70 mol of acid. Calculate the pH and the pOH of the…

A: Given, moles of H2SO4 = 0.70 mol Volume of the solution = 2.00 L pH of the solution = ? pOH of the…

Q: The pOH of 0.0260 M solution of Sr(OH)₂ is

A:

Q: Determine both the pH and the % ionization of a 0.53 M hypochlorous acid, HCIO, solution at 25°C.…

A: The given data is as follows: The concentration of HClO = 0.53 M The value of Ka for HClO = 2.9×10-8…

Q: A 0.54 M solution of chloroacetic acid, CICH2 CO2H, has a pH of 1.57. Calculate K, for the acid. %3D

A: Given: The molarity of the solution of chloroacetic acid = 0.54 M The pH of the solution = 1.57 We…

Q: Calculate the pH of the following solutions in which the [H+] is a) 0.01, b) 1.0 x 10 –8 , and c)…

A: Given that -  Hydrogen ion concentration , [H+] are -  a) 0.01 b)1.0 x 10 –8  c) 4.67 x 10 –4  Then,…

Q: The pH of a solution is 5.2, what is the [OH] concentration?

A: Given pH of the solution = 5.2 In order to find [OH-] concentration, we have to calculate pOH from…

Q: 4. If the molarity of hydrogen ions is 1.32(+0.02)x103 M, find the pH.

A: The molarity of hydrogen ion is given by 1.32 ±0.02 × 10-3 M.We have to calculate the pH of the…

Q: The pH of a 0.0040 M solution of HNO₃ is

A: The concentration of HNO3 is 0.0040M HNO3 is a monobasic acid. So, 1 mol HNO3 after dissociation…

Q: What is pH of a 0.1 Molar solution of oxalic acid in water

A: Given : Concentration of oxalic acid i.e H2C2O4 = 0.1 M The Ka1 and Ka2 of oxalic acid are 5.0 X…

Q: 2. The pH of a lime is 1.90. What is the [H3O*]?

A: pH is negative log of Proton concentration.

Q: What is the pH of an aqueous solution of 2.70×10² M hydrobromic acid?

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Q: The pH of a 0.224 M solution of a weak acid, HB, is 2.66. What is Ka for the weak acid?

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Q: What is the the PH and POH of the following solutions: 1. 0.05 M Ba(NO3)2 2. 0.01 M Na2SO4

A: The given solutions are 0.05 M Ba(NO3)2 and 0.01 Na2SO4.

Q: The pH of a lime is 1.90. What is the [H3O+]? What is the [-OH]?

A: Since the relationship between pH and  [H3O+] is  pH = -log[H3O+] and the relationship between pH…

Q: At the freezing point of water, Kw = 1.2 x 1015, What is the pH of ice water?

A:

Q: pH of a 0.223 M solution of sodium hydrogen chromate (K, 3.0 X 107)

A: Given data are as follows

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: Calculate the pH of a 2.61 mol/L solution of ammonium hydrogen carbonate, NH4HCO3

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Q: Determine the pH of a 1.2 M solution of ammonia, NH3, with K 1.8 x 105

A:

Q: What is the pH of an aqueous solution with a hydronium ion concentration of 1.75 × 10⁻⁵ M?

A: We know that, pH is the negative logarithm of hydronium ion concentration. i.e.,…

Q: Calculate the pH of the weak acid, lactic acid (HC3H5O3), if the concentration is 0.10 mol/L and the…

A: Given data,Molarity of lactic acid=0.10mol/LKa of lactic acid=1.4×10-4

Q: Write the formula for the conjugate acid of each of the following bases: (a) HS¯, (b) HCO,, (c)…

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Q: Calculate the pH of each of the following strong acid solutions: 0.225 g of HClO3 in 2.00 L of…

A: Strong acid dissociates completely when dissolved in water. The given acid HClO3 is a strong acid.…

Q: Calculate the pH of a solution which has a pOH of 7.2 (standard conditions)

A: Calculate the pH if pOH = 7.2

Q: If the OH− ion concentration of a blood sample is 6.7 × 10−7 M,  what is the pH of the blood…

A: pOH = -log [OH-] pH = 14 - pOH

Q: The pH of an aqueous solution of 0.175 M ammonium iodide, NH¼I (aq), is This solution is

A: Given : Concentration of NH4I = 0.175 M Since NH4I is made up of weak base NH3 and strong acid HI.…

Q: Question attached

A: pH is a measure of acidity of the solution. pH of a salt of a weak acid and strong base may be…

Q: A solution has a pOH of 12.4. What is the pH of this solution?

A:

Q: The pH of an aqueous solution of 0.223 M sodium hypochlorite, NaC1O (aq), is This solution is…

A: pH of salt produced from reaction of weak acid and strong base would be basic and pH of salt…

Q: Calculate the pH and pOH of the: 0.125M potassium hydroxide (KOH) solution

A:

Q: It is easy to measure the pH of a solution of a compound such as potassium hydrogen phosphate or…

A: The pH of a basic or an acidic solution is measured easily using pH meter. Calculating the pH of a…

Q: 6. The pH of a solution is 6.5, what is the [H3O*]? What is the pOH? What is the [OH]?

A: pH of solution is defined as the concentration of hydronium ion H3O+in the solution pOH of solution…

Q: If a 1.5 L sodium hydroxide solution contains 38g of NaOH, what is the pH of the solution?

A: We have to calculate the pH of Solution.

Q: The pH of an aqueous solution of 0.136 M sodium nitrite, NaNO2 (aq), is This solution is

A: NaNO2 is a salt of a weak acid (HNO2) and a strong base NaOH pH = 7 + (pKa + log C)/2

Q: What is the pH of a substance with a hydrogen ion concentration of 1.0 x 10-8 M?

A: Consider the given information is as follows: Concentration of hydrogen ion = 1.0×10-8 M     pH = ?

Q: The pH of a 0.0080 M solution of HNO₃ is

A:

Q: The hydrogen ion concentration of sulphuric acid is 0.01. Calculate its pH.

A: Given - Hydrogen ion concentration of sulphuric acid = 0.01 M

Q: Calculate the pH and pOH for 1.11M HCl solution?

A: To determined the concentration of dilute acids and dilute bases pH is introduced .    pH…

Q: The pH of orange juice is about 3.5. What would be the pOH of orange juice?

A: Given: pH= 3.5 pOH=? It is calculated as

Q: The pH of a 0.224 M solution of a weak acid, HB, is 2.63. What is Ka for the weak acid?

A:

Q: What are the pH and pOH of 0.075 M NaOH(aq)?

A: Since NaOH is a strong base Hence it will dissociate completely in solution  Since the dissociation…

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.