What is the pH of a 0.330 M solution of HF (Ka = 6.8 × 104)?

Q: If you have 0.1 x 6x 10^23 hydrogen ions in 1L of solution, what is the pH? O A. 7 В.3 O C. 5 O D.…

A: The correct answer is given below

Q: What is the pH of a solution that has [OH-] = 6.0 × 10−12 M?

A: pH: pH is  justified  as power of hydrogen. pH=-log[H+] Or in general we can say that it helps us to…

Q: What is the pOH of an aqueous solution of 0.315 M perchloric acid? pOH =

A:

Q: What is the pH of a 0.65 M solution of pyridine, C5H5N?

A: Given,  The concentration of C5H5N is 0.65M The kb value of C5H5N is 1.7×10-9 To solve: pH of 0.65M…

Q: What is the pH of a 0.00535 M solution of NaOH?

A: Number of moles of solute present in one litre of Solution is called Molality (M)  Units: mol/L  pH…

Q: Calculate the pH of a 5.6 x 10 M solution of HCIO4, a strong acid, at 25°C. pH =

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: 8. What is the pH of a cup of coffee that has a [OH-] of 1.200 x 10-10?

A: Detail mathematical calculation is shown below

Q: Given a diprotic acid, H₂A, with two ionization constants of K₁ = 4.5 x 104 and K = 2.2 x 10-12,…

A:

Q: Determine the pH of a 0.65 M solution of HCO₂K. The value of Ka for HCOOH is 1.8 × 10⁻⁴.

A: HCOOK is a salt of a weak acid (HCOOH) and a strong base (KOH). The salt is present as HCOO- and K+…

Q: Find the pH of a solution whose [OH] is 2.8 x 10 5 M. O 2.8 O 9.4 O 4.6 O 13

A: Using relation between pH and pOH we can find pH.  Given [OH-] = 2.8 * 10-5M

Q: What is the pH of a solution with a hydrogen concentration of 8.6x10-2M?|

A:

Q: Calculate the pH of a 1.5 x 10-2 M solution of HBr.

A: The concentration of HBr solution is = 1.5 x 10-2 M The pH of the solution is =?

Q: what is the pH of a 0.00761 molar solution of HNO3?

A: Nitric acid is a strong acid that dissociates completely in aqueous solution.

Q: 4. A certain brand of rootbeer has a hydrogen concentration equal to 1.9 x 10 M. What is the pH and…

A: pH =-log[H+]  pOH = -log[OH-]

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=1.6×10^−4 M?   pH=

A: The pH of an aqueous solution can be calculated using equation (1). In this equation [H+] represents…

Q: calculate ph of 7*10^-3 M aqueous solution of Ca(OH)2 at 25 degrees

A:

Q: What is the pH of a 7.7 x 10® M KOH solution?

A: Here ,the concentration of KOH is less , so we can not neglect the concentration oh OH- comes from…

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: If the hydroxide concentration of a solution is [OH-] = 4.67 X 10-8 what would the pH of that…

A: Given:The concentration of OH, [OH-] = 4.67 X 10-8To find:pH = ?

Q: calculate the pH of a 0.10 M perchloric ,HCIO4, solution.

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration, [H+] expressed in mol/L…

Q: What is the pH of a 0.015 M Ba(OH)2 solution?

A:

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: Calculate the pH of a 7.1 x 104 M solution of HC104, a strong acid, at 25°C. pH =

A:

Q: Find the pH of a 0.337 M aqueous solution of hydrofluoric acid (HF), for which Ka = 6.8 × 10–4.

A: Weak acids :-  Acids which do not undergo complete dissociation and produce very less number of H+…

Q: the concentration of H3O+ of seawater is 3.16 x 10-9. what is the pH of seawater?

A: Ph depends on concentration of H+ ions...

Q: What is the pH of a solution with molar concentration of Ht, [H*] = 1.0 x 10-9 M?

A:

Q: What is the pH of the following solutions? [OH-] = 9.1 × 10-3 M

A: We can only Calculate the pH of solution if we know the Hydrogen ion concentration of solution. To…

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: What is the pH of a solution that has [OH-] = 2.2 x 10-5 M?

A:

Q: What is the PH of 1.25 x 10-6 M HCI solution?

A:

Q: If the [OH-] is 3.5 x 10 then what is the pH of the solution?

A: Given, [OH-] = 3.5 x 10-5  PH = ?

Q: Determine the pH of a 1.00×10¯7 M aqueous solution of HBr.

A: Given : concentration of HBr solution = 1.00 × 10-7 M  To calculate :- pH of solution

Q: What is the pH of a 0.00205 M solution of NaOH?

A:

Q: Given that the Ka of a monoprotic acid HA is 3.20 x 10, and the acid HA concentration is 0.751 M,…

A:

Q: what is the pH of a 7.5x10^-2 M solution of NaOH?

A:

Q: A solution has an OH⁻ concentration of 1.3 x 10⁻⁴. What is the pH of the solution at 25°C?

A: pH = -log [H+] [H+][OH-] = 1 x 10-14     at 25°C

Q: How many moles of NH3 must be dissolved in water to give 615.4 mL of solution with a pH of 10.96? K…

A: The number of moles NH3 disolved in water is given below

Q: Determine the pH @ 25 ºC of a solution that has [OH−] = 2.5 x 10−9 M.

A:

Q: what is the pH of a 7.1 x 10^-3 M solution of H^+?

A: Given : [H+ ]  = 7.1  x 10-3 M

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

A:

Q: What is the pH of a 0.0128 M solution of Sr(OH)2 solution?

A: pH can be defined as the potential of the hydrogen. It is the measurement of how acidic or basic the…

Q: What is the pH of a 5.3 x 10^-6 M HBr solution?

A:

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: What is the pH of a solution with a [H] of 3.5 x 10³? (K)

A:

Q: What is the pH of a 6.9 × 10⁻⁶ M KOH solution?

A: Use formula POH= -log(OH-) PH+POH=14 PH= 8.84

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

A:

Q: What is the pH of a 0.76M solution of Ba(OH)2?

A: We have to calculate the pH of 0.76 M solution of Ba(OH)2

Q: Determine the pH of an aqueous solution where [OH] = 6.0 x 10 10 M.

A: Given data : [OH-] = 6.0 × 10-10 M.  To find : pH

Q: Calculate the pH and pOH of a 4.3 x 10-3M solution of NaOH.

A: Given information: Concentration of NaOH = 4.3 x 10-3M

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.