What is the pH of a 0.580 M solution of C3H,NHB (Kb of CsH;N is 1.7 × 10-º)?

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 5.0×10-2 M solution of KOH at 25 °C?

A:

Q: HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.054M in…

Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in base…

A: pH is the measure of concentration of H+ ions. Here pH can be calculated with the help of kB values,…

Q: What is the pH of a 0.0810 M solution of HONH;CI (Kb of HONH2 is 1.1 x 108)?

A: Given,                HONH3Cl -----> HONH3+ + Cl-  Hydrolysis of the weak conjugate acid, HONH3+…

Q: CH3NH2 is a weak base (?b=5.0×10^−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a…

A: CH3NH3NO3 → NO3- + CH3NH3+ Kb for the above reaction is 5x10-4  CH3NH3 can donate a proton and…

Q: What is the pH of a 0.083 M solution of NaCN?

A: Given :- Concentration NaCN solution = 0.083 M  To calculate :- pH of solution

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

A:

Q: Do you think the pH of 1.0 M tri-methyl ammonium (CH3)3NH", pKa 9.80, will be higher or lower than…

A:

Q: What is the pH of a 0.0520 M solution of HONH;CI (Kb of HONH2 is 1.1 x 10-8)?

A: HONH3Cl is a salt of weak base HONH2 and strong acid HCl Recall the following expression to…

Q: What is the pH of a solution consisting of 0.70 M HC2H3O2 and 0.60 M NaC2H3O2 ? The Ka of HC,H3O2 is…

A:

Q: What is the concentration of a solution of (a) KOH for which the pH is 11.89, (b) Ca(OH)2 for which…

A: We use the PH equation for calculation for H+ concentration.  Then apply Ionic  product  of water to…

Q: What is the [oh-] of an aqueous solution with a ph of 11.45?

A: C2H6. An acidic substance is the substance that can give H+ ions. They are corrosive and sour in…

Q: The pOH of ammonium hydroxide at 25 C is 5.55. What is the pH and the [H ], [OH ] in mol/L for…

A: At constant temperature, the pH of a solution remains constant. For 250 C, the pH of the solution…

Q: What is the pH of a 6.59×10-3 M  aqueous solution of hydrochloric acid?

A:

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.450 M  solution of methylamine?

A: Methylamine, CH3NH2 is a weak base which undergoes partial dissociation in aqueous medium. Let the…

Q: What is the pH of a 3.6×10-2 M solution of KOH at 25 °C?

A:

Q: What is the pH and concentration of OH- of 0.0200 M CH3COOH?

A: Given,Concentration of acetic acid is 0.0200M.Ka = 1.8×10-5.The equation will be:

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

A:

Q: What is the pH of a solution that is 1 × 10-8 M with respect to H+?

A: Here given, Concentration of H+, that is [H+] = 1 x 10-8 M We know, that---- PH = - log [H+]

Q: In an aqueous solution at 25 C, if [H3O+]=3.1×10^-4M, then [OH-] is

A: Given data: The hydronium ion concentration is H3O+=3.1×10-4 M. To find: The hydroxide ion…

Q: HClO is a weak acid (?a=4.0×10^−8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Given : Concentration of NaClO = 0.014 M Since NaClO is a weak conjugate base of weak acid HClO.…

Q: What is the pH of a 0.0011M solution of Ca(OH)2?

A: Calcium hydroxide is a strong base. It undergoes complete dissociation in water to give two moles of…

Q: What is the molar concentration of a weak acid [HA], if the ka = 6.34 x 105 and the [H*] = 9.77 x…

A: Dissociation of weak acid :   HA  ⇌H+ + A-

Q: When [H+] = 4.0 × 10-9 M in water at 25°C, what is the pH?

A:

Q: When [H+]=4.0 x 10(-9) M in water at 25 C, what is the pH

A: Given that Concentration of H+ = 4.0×10-9 M

Q: What is the pH of a 3.9×10-2 M solution of KOH at 25 °C?

A: KOH ionizes in aqueous solution as,                          KOH (aq)       -----> K+ (aq)   +…

Q: What is the pH of a 0.380 M solution of NACN (Ka of HCN is 4.9 x 1010)?

A:

Q: Calculate the pH of an aqueous solution at 25⁰C that is (b) 0.035 M in HClO4 (c) 1.5×10-6 M in HCl.

A: PH = -log [H+]  HClO4 and HCl are strong acid so concentration of H+  ion  concentration..

Q: A diprotic acid, H:A, has Ka1 = 3.4 × 104 and Ka2 = 6.7 × 10-°. What is the pH of a 0.17 M solution…

A:

Q: What is the pH of (3.21x10^-1) M C5H5NHBr?

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: What is the pH of a 8.1 × 10-6 M KOH solution?

A: The pH scale is introduced by the scientist Sorensen in order to express the [H3O+] ion of a…

Q: 1. HOW DO WE FIND THE pH, H+ and OH- of a 0.10 M KAI(SO4)2.

A: Given concentration of KAl(SO4)2 is 0.10M

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 2.4 × 10⁻⁴ M, then [OH⁻] is:

A: we have, [H3O+] =2.4 x10-4 M To calculate the concentration of OH-, firstly calculate the PH  of the…

Q: HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: It is required to calculate the pH of the solution that is 0.016 M in NaClO.Ka for HClO = 4 x 10-8…

Q: The pH of a 0.501 M  solution of the conjugate base, A-, of a weak acid, HA, is 11.10. What is the…

A: Given: pH = 11.10 [A-] = 0.501 M As pH = -log[H+] Thus,  [H+] = 10-pH = 1011.10 = 7.9 x 10-12 M…

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 10.3 O 12.7 O 11.5 O 13.1 O13.8

A: pH of solution is calculated using relation pH + pOH = 14

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4.  What is the pH of a 0.290 M  solution of methylamine?

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

A:

Q: Why is the pH of water at 25oC equal to 7.00?

A:

Q: What is the pH of a 4.5×102M solution of KOH at 25 °C?

A: Given:   The concentration of KOH is 4.5×10-2 M. The value of temperature is 25 ˚C.

Q: ph of 0.10 M NaNO2 (Ka of HNO2 is 4.5 x 10-4 ?

A: Given information: 0.10 M NaNO2 Ka of HNO2 is 4.5 x 10-4

Q: The hydroxide ion concentration of an aqueous solution of 0.532 M phenol (a weak acid), C,H;OH, is…

A:

Q: What is the pH of a solution containing 0.055 mol L-1 HCOOH and 0.141 mol L-1 HCOO- ?

A:

Q: HClO is a weak acid (?a=4.0×10−8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: An acid is a substance that can furnish the hydrogen ions in the aqueous solution. The weak acid…

Q: What's the pH of a solution with an H+ concentration of: 1.247 x 1012, Round to 2 decimal places.

A: Value of pH is used to measure the acidity or basicity of a solution. At room temperature, value of…

Q: Calculate the pH of a 0.400 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4.

A:

Q: What is the pH of a 0.89x10-2 M solution of Ba(OH)2 at 25°C?

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.