What is the pH of a 1.8x10 molar aqueous nitric acid solution? (Hint: The H,0* due to the water ionization is not negligible here.)

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: Calculate the pH of a 1.88 M NH3 (Kb = 1.8 x 10^–5) solution

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: The pH of a 1.00 × 10² M solution of cyanic acid (HOCN) is 2.77 at 25.0 °C. Calculate Ka for HOCN…

A: Solution :         The process of dissociation involves the segregation of molecules into smaller…

Q: What is the pH of a 1.00x 10 molar solution of LICI? Report your answer with 2 places past the…

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Q: The Ka, for propionic acid, HC3H5O2, is 1.30 x 10^ -5. What is the pH of a 0.0850 M propionic acid…

A: The dissociation reaction of propanoic acid is given by  HC3H5O2 -----> H+ + C3H5O2- hence Ka = […

Q: A 1dm3 aqueous solution contains 5.80g of sodium hydroxide, NaOH.  What is the pH of the solution at…

A:

Q: Enter your answer in the provided box. Determine the K, of a weak base if a 0.29 M solution of the…

A: The pOH of 0.29 M solution is calculated below.

Q: If an acid, HA, dissociates to 0.1% when added at a final concentration of 0.05M in water, that is:…

A: 1- First calculate the H3O+ ion concentration :  [H3O+] = ( Concentration ) × ( Degree of…

Q: What is the pH of a solution that is 2.0 M HF and 2.0 M F–?  Does your answer make sense?

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: Calculate the pH of a 0.0010 M solution of HB, a hypothetical acid with K-9.6 x 10. (Use the method…

A: The pH of 0.0010 M HB solution is calculated as shown below. H+=KaC=9.6×10-5×0.0010 M=3.10×10-4 M

Q: What is the pH of 3.78 *10^-2 M nitric acid in aqueous solution ?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

Q: What is the pH of an aqueous solution of 1.45×10-2 M nitric acid?

A: Nitric acid i.e HNO3 is a strong acid. Hence it dissociates into ions completely as per the…

Q: What is the pH of a solution of 5.94 M of HASO, which has K,= 5.1 x 10- Round and report your answer…

A: Concentration of H3AsO3 is 5.94 M. The value of acid dissociation constant is 5.1×10-10.

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

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: 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 0.25 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic acid,…

A:

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: If the pH of a 25 °C NaOH solution is 9.00, what is the molarity of NaOH in that solution?

A:

Q: 6. [H*] for = 1.57x10 M, what is the [OH]?

A: pH is quantitative measure of the acidity or basicity of aqueous  solutions. This is widely used in…

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

A:

Q: The [OH–] = 1.3 x 10–6 M for a 0.025 M solution of a weak base. Calculate the value of Kb for this…

A: Kb value for given weak base is 5.2×10^-5.

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: 6.7 x 10, What is the pH of A solution at 25 °C has [OH] = the solution?

A: Number 1 :- Given :- [OH-] = 6.7 × 10-3  To calculate :- pH of solution

Q: The pH of an acetic acid (Ka = 1.75 x 10−5) solution is 3.14.  What is the concentration of acetic…

A: Given :-  pH of acetic acid solution = 3.14  Ka for acetic acid = 1.75 × 10-5  To be calculated :-…

Q: Calculate the percent ionization of a 0.125-M solution of nitrous acid (a weak acid), with a pH of…

A: pH of a solution is equal to negative logarithm of the concentration of the hydrogen ion. Write the…

Q: (1point) Calculate the pH and pOH of a 4.3 x 10 M solution of NaOH.

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: 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: Find the pH of a 0.250 M NaC2H3O2 solution.

A: The dissociation reaction with ICE TABLE C₂H₃O₂⁻ + H₂O ⇄ HC₂H₃O₂ + OH⁻ I 0.250 C -x +x +x E 0.250-x…

Q: What is the pH of an aqueous solution with a hydroxide ion concentration of 4.20 x 10-4 M?

A:

Q: Question is attached

A: Given information: Concentration of dimethylamine = 0.393 M

Q: What is the pH of a solution that is prepared by adding 4.0 mL of 0.50 M NAOH(aq) and 4.0 mL of 0.40…

A:

Q: weak base is 2.5 × 10-6, what is the pH of a 0.23 M solution of this base?

A: From the relation, pOH is calculated as,

Q: Calculate the pH of an aqueous solution of 6.45×10-2 M sodium sulfite.   pH = ?

A: Sodium sulfite is salt of mixture of strong base sodium hydroxide(NaOH) and weak acid sulfurous…

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

A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.029M in…

Q: NH3 is a weak base (?b=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

A:

Q: The pH of a 0.20-M solution of HF is 1.92. Determine Ka for HF from these data.

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

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: Determine the pH of 3.15 M HF. For HF, Ka = 6.5 x 104

A:

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

A:

Q: Calculate the pH of a solution made by adding 2.70 g of lithium oxide (Li2O) to enough water to make…

A: Mass of lithium oxide = 2.70 g Volume of solution = 1.300 L

Q: What is the pH of a 4.5 x 10-7 M solution of NaOH?

A: Answer :- pH = 7.65  The pH of  4.5 × 10-7 M NaOH solution = 7.65…

Q: How many grams of NaHCO3 must be added to 4 g K2CO3 to give a pH of 10.80 in 500 ml total solution?

A: Henderson-Hasselbach equation is given by: pH = pKa + logA-HAwhere [HA] is the concentration of the…

Q: A 0.051 M weak acid solution, HA, has a pH of 1.95. What is the Ka of the acid

A: [H+]  = (Ka  × C )1/2

Q: What is the pH and the concentrations (of all species) in a 0.075 M solution of Na2S?

A:

Q: NH3 contains no OH- ions, and yet its aqueous solutions are basic. Explain why?

A: According to Lewis concept Ammonia is considered as base since it has lone pair of electrons with…

Q: Enter your answer in the provided box. Calculate the pH at 25°C of a 0.045 M solution of a weak acid…

A: The acid dissociation constant for the weak acid is = 1.6×10-5 The concentration of weak acid…

Q: Acetic acid (CH,COOH, Ka = 1.80 x 10-5) is a weak acid, so the salt sodium acetate (CH,COONA) acts…

A: In the given question we have to calculate the pH of 0.384 M sodium acetate. the given ka of acetic…

Q: Explain how you determine the pH of 0.500 M HOCI (Ka 3.6 x 108)

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…

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.