What is the pH of a 0.750 M solution of C,H,NHB (Kb of C,H̟N is 1.7 10°)?

Q: What is the original molarity of a solution of ammonia whose pH is 10.48?

A: The original molarity of solution of ammonia whose pH is the 10.48 is calculated as follows

Q: What is the pH of a 0.660 M solution of NaCN (Ka of HCN is 4.9 × 10⁻¹⁰)?

A: The pH will be 11.56.

Q: What is the pH of a 0.570 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?

A: NaCN dissociates in an aqueous medium as follows: NaCN→Na++CN- Na+ ions don't contribute to the pH…

Q: If the K, of a weak base is 7.2 × 10-6, what is the pH of a 0.33 M solution of this base? pH =

A: in this question given data is  α=KaC   ka×kb=10-14C=0.33MPH=-logH+ Apply the value given formula,…

Q: The pH of a 0.205 M solution of a weak acid, HB, is 2.58. What is K, for the weak acid?

A: The given data is as follows: The pH of solution = 2.58 The concentration of weak acid, HB = 0.205 M…

Q: 4. A 0.020 M weak acid HA, has a pH of 3.21. What is the Ka of the acid?

A:

Q: A)The pOH of a 0.250 M solution of NaOH is?   B)The pH of a basic solution is 10.59. What is pOH?

A: pH - pH is defined as negative logarithm to the base 10 of H+ ion concentration. Mathematically, pH…

Q: 2. The pH of .010 M HX, a weak acid, is 4.44 a. Calculate the pOH b. Determine its percent…

A: pH = 4.44 Concentration of HX = 0.01 M

Q: HCN is a weak acid (Ka=6.20×10−10), so the salt, KCN , acts as a weak base. What is the pH of a…

A: Ka = 6.20×10-10 pKa = -log(Ka)    = -log(6.2×10-10 = 9.21  Concentration(C) of salt =0.0750 M

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.15. What is the Kb of this base?

A: Solution:       Weak bases on dissociation show partial ionization. This means that an equilibrium…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.63. What is the Kb of this base?

A: The weak base dissociates feebly in an aqueous solution to furnish the hydroxide ions. For example,…

Q: A solution of sodium acetate (NaCH3COO0 has a pH of9.70. What is the molarity of the solution?

A:

Q: What

A: We will use concept of pH of salt

Q: The pH of a 0.154 M solution of a weak acid, HB, is 2.72. What is K, for the weak acid?

A:

Q: The [OH] of a solution that has a pH of 6.75 at 25°C is ..

A: Solubilty  product  constant determines the solubilty of ions in solution.

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.54. What is the Kb of this base?

A: pH = -log[H3O+] Where [H3O+] is the concentration of hydronium ion…

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 11.90. What is the Kb of this…

A: Given: Concentration of base = 0.0910 M And pH of solution = 11.90  Since pOH = 14 - pH => pOH =…

Q: What is (a) the pH, and (b) the percent ionization of 0.62 M propionic acid, HC3H5O2? (ka for…

A: Given: Molarity of propionic acid= 0.62 M

Q: What is the pH of a 0.580 M solution of NaCN (Ka of HCN is 4.9 x 1010)?

A:

Q: The pH of a 0.206 M solution of a weak acid, HB, is 2.59. What is K, for the weak acid?

A: pH = 2.59 pH = -log [H+]2.59 = -log [H+] [H+] = 10-2.59   Relationship between the dissociation…

Q: What is the pH of a 0.250 M HOCI solution? K, of HOCI at 25°C is 3.5 x 10-8. O 7.46 O 4.03 O 3.57 O…

A: ​Given - - - >   Ka = 3.5*10-8   pH = 0.25

Q: What is the pH of a solution that contains 0.561g of dissolved KOH in 10.0L of aqueous solution?

A: Mass of KOH =0.561 g Volume of solution = 10 L Molar mass of KOH = 56.10 g/mol pH of solution = ?

Q: Methylamine, CH3NH2, is a weak base. In 0.200 M CH3NH2, only 8.4 % of the base has undergone…

A:

Q: A 0.050 M solution of a weak acid (HA) has a pH of 4.70. What is the Ka of the acid?

A: We will have the below reaction taking place. HA ----> H+ + A- Since pH = -log[H+] where [H+] =…

Q: The PH in a 0.050 M solution of Ba(OH)2 is:

A: pH in 0.05M of Ba(OH)2 is determined as

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.80. What is the Kb of this…

A: Welcome to bartleby!  Introduction :  We have to calculate Kb of the base .

Q: Suppose that a benzoic acid (C,H,COOH) solution has a pH of 3.15. Which of these substances would…

A: Given substances: KCl C6H5COONa NaI HBr We have to find the substance that would increase the pH…

Q: What is the pH of a 0.730 M solution of NaCN (Ka of HCN is 4.9 × 10⁻¹⁰)?

A: Interpretation: The pH of a 0.730 M solution of NaCN is to be determined. Ka of HCN = 4.9 × 10-10

Q: HCN is a weak acid (Ka=6.20×10−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: Weak acid are those acid which does not dissociate completely in aqueous solution and weak base are…

Q: 1. Arrange the following in order of increasing pH of their corresponding solutions. a. CH;NH;CI,…

A: Given,  a. CH3NH3Cl, NaCH3COO, RbBr  b. K2C2O4 , C2H5NH3Br, Ba(ClO4)2  Arrange the following…

Q: dissociated H+H+ ions

A:

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 12.30. What is the Kb of this…

A:

Q: What is the pH of a 0.0380 M solution of HONH,CI (Ka of HONH,+ is 9.1 × 10-7)?

A:

Q: What is the pH of a solution that is 0.071 M LiCN at 25°C?

A: A solution is made up of 0.071 M LiCN at 25 ◦ C. Here, we have to calculate the pH of the solution.…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.64. What is the Kb of this base?

A:

Q: The pH of a 0.229 M solution of a weak acid, HB, is 2.50. What is K, for the weak acid?

A: Given :-  Concentration of weak acid HB = 0.229 M  pH of solution = 2.50  To calculate :-  Ka for…

Q: What is the pH of a 0.690 M solution of NACN (Ka of HCN is 4.9 x 10 10)?

A: Given, The concentration of the solution of NaCN = 0.690 M Acid dissociation constant (Ka) = 4.9 x…

Q: The pH of a 0.220M solution of a weak acid, HB, is 2.51. What is Ka for the weak acid?

A: Given  PH of weak acid = 2.51  Concentration of weak acid ( c ) = 0.220 M  Ionization constant ( Ka…

Q: Calaiste t PH and the POH FOR a 06 M Solution of Ca(OH)₂

A:

Q: Whats pH of a solution that is 0.010 M in HClO Ka = 3.5 × 10–8 and 0.010 M in HCl?

A: Since HCl is a strong acid, it is completely dissociated into H+(aq) and Cl-(aq).  Hence [H+(aq)] =…

Q: HA weak acid has (K = 0.0056), a concentration of 0.480 M. what is pH of the acid

A: Weak acid dissociate less in solution

Q: What is the pH of a solution prepared by adding 0.253g of ammonium chloride to 0.241ml of water? Kb…

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: A 0.025 M solution of a weak acid (HA) has a pH of 4.28. What is the K, of the acid? a

A: ka is the ratio of  product of concentration of products raised to their stoichiometric coefficient…

Q: The pH of a solution that has measured (H+) of 6.8*10^-9 M is

A: We have given that   [H+] = 6.8×10-9M  pH is measure the acidity and basicity of aqueous…

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 11.20. What is the Kb of this…

A:

Q: _s the pH of an aqueous solution that is 0.1M NH4C1?

A:

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.37. What is the Kb of this base?

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: What is the pH of a 0.200 M NaHCO, solution? The K, for HCO, is 5.6 x 1011

A:

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.53. What is the Kb of this base?

A: The K b represents an equilibrium constant.  If the value of K b is small, then the base will be…

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.