If the Kp of a weak base is 3.4 × 10-0, what is the pH of a 0.25 M solution of this base? pH =

Q: A 0.010 M solution of a weak acid, HA, has a pH of 3.10. What is the K, of the acid? 6.3 x 106 6.3…

A: pH is the negative logarithm of the hydronium ion concentration of a solution. Given:- pH = 3.10…

Q: What is the pH of a solution of 8.2 x 10-5 M HCl?

A: GivenConcentration of HCl = 8.2 x 10-5 MHCl a strong electrolyte completely dissociate solutionHCl →…

Q: The pH of a solution containing a hydrogen ion concentration of 1 x 10-5 is 5 and its pOH is 9,…

A: Given that:  [H+] = 1×10-5 pOH = 9  using relation  pH = -log[H+]

Q: If the K of a weak base is 8.5 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

A:

Q: 2. 50 x 10-5 , wha

A: Given data are as follows: Concentration of acidic solution = 0.05 M Ionization constant = 2. 50 x…

Q: If the Ka of a monoprotic weak acid is 5.8 × 10-6, what is the pH of a 0.47 M solution of this acid?

A: Given: Ka=5.8×10-6 Molarity of acid = 0.47 M

Q: what is the ph of a solution that is 0.100 m in hydrofluoric acid? The Ka of hydrofluoric acid is…

A: Recall the following expression to find pH of the given solution of hydrofluoric acid. Given that…

Q: A certain weak base has a Kp of 7.30 x 10-'. What concentration of this base will produce a pH of…

A: Given data, Kb =7.30×10-7 pH =10.37 Let us consider the weak base is B. It react with water as,…

Q: What is the pH of a solution containing 0.225 M weak base, B', with a K, of 3.8 X 10-7? в (аq) + Н,О…

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Q: For a given acid, Ka is 7.2  x 10−4. This means that it is: a strong acid B a weak base C a weak…

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Q: If the K of a weak base is 7.0 × 10-6, what is the pH of a 0.37 M solution of this base? pH :

A: We make an ICE table then equilibrium constant expression is written ,since we have weak acid so we…

Q: Calculate the pH and the pOH of these solutions:   (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH =   pOH…

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Q: What is the pH of a 0.17 M weak acid solution? The KA of the weak acid is 2.1 x 10-5.

A: Given :-  Initial concentration of weak acid = 0.17 M  Ka for acid = 2.1 × 10-5  To be calculated :-…

Q: If the Ka of a monoprotic weak acid is 5.8 x 10-6, what is the pH of a 0.12 M solution of this acid?

A: Negative logarithm of Concentration of [H+] ion present in the solution is known as pH of the…

Q: Which of the following aqueous solutions has the highest pH? a) 0.10 M HCI b) 0.10 M HCIO c) 0.10 M…

A: Given options are : a). 0.10 M HCl  b). 0.10 M HClO  c). 0.10 M HCl in 0.10 M KCl  d). 0.10 M HClO…

Q: If 34.6 mL of a 0.68 M NaOH solution is added to a 51.9 mL sample of a 0.68 M weak acid, HA , what…

A: 34.6 mL of a 0.68 M NaOH solution is added to 51.9 mL sample of a 0.68 M weak acid, HA (ka = 1.8 x…

Q: If the Ka of a monoprotic weak acid is 3.4 × 10-6, what is the pH of a 0.30 M solution of this acid?

A: The dissociation of a weak acid is written as:

Q: Ammonia is a weak base that is a household cleaner and has a Kb =1.8 x 10-5. What is the pH of a 3.0…

A: Given: Kb =1.8 x 10-5Concentration = 3.0 M pH = ?

Q: A weak base has a base hydrolysis constant, K, of 3.2 x 10-6. What is the pH of a 0.18 M solution of…

A:

Q: What is the pH of a soln which  is 0.5 M NH3 and 0.075M NH4Cl? (kb=1.8x10-5)

A: The solution of NH3 and NH4Cl will form a buffer solution and the pH of a buffer solution is…

Q: If the K of a monoprotic weak acid is 1.8 x 10-6, what is the pH of a 0.35 M solution of this acid?

A: Given: Ka of weak monoprotic acid (Assuming HA) = 1.8 × 10-6  And the concentration of HA = 0.35 M

Q: The ionization constant for NH3 in water is 1.8 x 10 - 5. Determine the hydrox concentration and the…

A: The dissociation of ammonia in aqueous solution can be represented as: The ionization constant for…

Q: If the K, of a monoprotic weak acid is 1.4 x 10-6, what is the pH of a 0.14 M solution of this acid?…

A: Given:   The concentration of acid is 0.14 M. The Ka of a monoprotic weak acid is 1.4×10-6.

Q: Calculate the pH of a solution that is 0.54 M HF and 1.00 M KF. Ka = 7.2x104 pH =

A: Given, Concentration of HF = 0.54 M Concentration of KF = 1.00 M Ka for HF = 7.2 x 10-4  PH = ?

Q: The pH of a 0.10 M solution of a monoprotic acid is 2.85. What is the value of the ionization…

A: Given data is as follows: The concentration of monoprotic acid = 0.10 M The pH of the solution =…

Q: If the K of a monoprotic weak acid is 1.4 x 10-6, what is the pH of a 0.14 M solution of this acid?…

A: Given : Ka of monoprotic acid (assuming HA) = 1.4 X 10-6  And Concentration of acid = 0.14 M Since…

Q: The K, of a weak monoprotic acid is 1.65 x 10-5. What is the pH of a 0.0859 M solution of this acid?…

A: In this question, we want to determine the pH of the weak monoprotic acid,  How we can determine the…

Q: Based on the Kb determined in the previous part, what is the pH of the initial 1.0 M base solution?…

A:

Q: If you dissolved the salt ammonium cyanate, NH4(NCO), in water, what type of solution would you…

A: Ammonium cyanate [NH4(NCO)] is salt of weak base NH3 and weak acid HNCO Ka of HNCO = 2×10-4 pKa =…

Q: If the K, of a weak base is 2.4 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

A: Given,  Base dissociation constant of base (say B) = Kb= 2.4 x 10-6  Molarity of base (B) = 0.27 M…

Q: Calculate the molar concentration of OH- in a water solution that has a molar concentration of H+…

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Q: HCN has a K, of 4.9 X 10-10. What is the pH of a solution which contains 0.350 M NaCN? CN (aq) + H,O…

A: The pH of a solution helps to determine the acidity and alkalinity of a solution. The solution maybe…

Q: The K₂ of a weak monoprotic acid is 1.74 x 10-5. What is the pH of a 0.0939 M solution of this acid?…

A:

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: If the K of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH =

A:

Q: What is the K w of pure water at 15.0°C, if the pH is 7.20 ? 1.00 x 10^-14 6.31 x 10^-8 1.26 x…

A: Given , PH = 7.20  Kw = ?

Q: If the Ką of a monoprotic weak acid is 1.4 × 10-6, what is the pH of a 0.42 M solution of this acid?…

A: Given data, ka = 1.4 × 10-6  Concentration of Weak acid = 0.42 M

Q: Calculate the pH of a solution that is 0.450 M HC2H2O2 and 0.730 M NaC2H3O2. The Ka for acetic acid…

A: This problem is solved by using Henderson Hassel baltch equation.

Q: what is the pH of a blood sample with a molar mass concentration of H+ ions as 7.2x 10^-8

A:

Q: If the Ka of a monoprotic weak acid is 1.3 x 10-6, what is the pH of a 0.18 M solution of this acid?…

A:

Q: What is the pH of a solution of HCl with concentration of 3.5 × 10-3? Make sure to choose the answer…

A: The pH of solution is calculated using the concentration of hydrogen ions, which indicates the…

Q: If the Ka of a monoprotic weak acid is 1.6 x 10-6, what is the pH of a 0.37 M solution of this acid?…

A:

Q: What is the pH of a solution of 0.12 M HOCl and 0.53 M NaOCl? Ka = 3.5x10-8

A: Given, Concentration of HOCl = [HOCl] = Concentration of NaOCl = [NaOCl] = Ka for HOCl = 3.5 × 10-8…

Q: What is the hydronium ion concentration in 0.0200 M HClO?   Ka = 2.88 x 10-8

A: In order to calculate the concentration of the hydronium ion we first write down the given data:…

Q: The Ka of a weak monoprotic acid is 1.13 x 10-5. What is the pH of a 0.0777 M solution of this acid?…

A:

Q: If the Ka of a monoprotic weak acid is 4.7 x 10-6, what is the pH of a 0.49 M solution of this acid?…

A: Given Ka = 4.7 x 10-6 C = 0.49 M

Q: A student is asked to calculate the pH of 10-3  M NaCl solution. The student answers, "3." What is…

A: Salt are produced by the reaction of an acid and a base. For example, The pH of salt is given as :…

Q: Determine the pH of a 0.068 M aqueous solution of sodium cyanide. The Ka for HCN is 4.9x 10^-10

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.