An unknown weak acid with a concentration of 0.080 M has a pH of 1.80. What is the Ka of the weak acid?

Q: An unknown weak acid with a concentration of 0.530 M has a pH of 5.600. What is the Ka of the weak…

A: Given, Concentration of the unknown weak acid (C) = 0.530 M pH of the solution = 5.60  Ka for weak…

Q: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: A 0.035 M solution of a weak acid (HA) has a pH of 4.88.What is the Kₐ of the acid?

A:

Q: An unknown weak acid with a concentration of 0.350 M has a pH of 5.600. What is the Ka of the weak…

A: given, the concentration of weak acid (c) = 0.350M pH = 5.600

Q: A 0.0722 M solution of a weak acid has a pH of 3.11. Calculate the Ka of this acid.

A: A weak acid is an acid that dissociates partially to give H3O+ in water. The dissociation of a weak…

Q: The pH of 0.259 M solution of an unknown acid is measured to be 2.353. What is the Ka of the acid?

A:

Q: An unknown weak acid with a concentration of 0.310 M has a pH of 5.600. What is the Ka of the weak…

A: Give data, Molarity of HA = 0.310M pH = 5.600 Equilibrium constant is defined as the ratio of…

Q: A solution of a weak acid has a concentration of 0.64 M and is found to have a pH of 3.77. What is…

A: The dissociation of a weak acid can be depicted as follows.           HA   +H2O ⇔    A-  +  H3O+I…

Q: An unknown weak acid with a concentration of 0.077 M has a pH of 1.80. What is the Ka of the weak…

A: The Ka of weak acid

Q: The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31.  What is the Ka of the acid?

A: Given  pH = 2.31 Concentration of acid = 1.86 M Ka =?

Q: A 0.037 M solution of a weak acid (HA) has a pH of 4.34. What is the Ka of the acid?

A:

Q: An unknown weak acid with a concentration of 0.320 M has a pH of 5.600. What is the Ka of the weak…

A: HA  ↔ H+ + A-Writing equilibrium expression for the above weak acid,Ka = [H+] [A-][HA]  But at…

Q: An unknown weak acid with a concentration of 0.130 M has a pH of 5.600. What is the Ka of the weak…

A: Assuming the unknown weak acid is HA Hence the dissociation reaction of acid is  HA ------> H+ +…

Q: Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80.

A:

Q: concentration

A: [H+] = 10^-pH  [H+] = 10^-1.80  [H+] = 0.0158 M

Q: An unknown weak acid with a concentration of 0.290 M has a pH of 5.600. What is the Ka of the weak…

A: For weak acid,pH=12(pKa-logC)Where, C is concentration in M unit

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 of 0.0720M solution of a weak acid is 2.670. What is the Ka of the acid

A:

Q: An unknown weak acid with a concentration of 0.063 M has a pH of 1.80. What is the Ka of the weak…

A: Given: An unknown weak acid with a concentration of 0.063 M has a pH of 1.80. We have to calculate…

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: An unknown weak acid with a concentration of 0.071 M has a pH of 1.80. What is the Ka of the weak…

A: [acid]=[HA]=0.071MpH=1.80Ka=?

Q: A weak acid is dissolved in water to generate a solution that is 0.100 M. The pH of this solution is…

A:

Q: An unknown weak acid with a concentration of 0.085 M has a pH of 1.80. What is the Ka of the weak…

A:

Q: An unknown weak acid with a concentration of 0.190 M has a pH of 5.600. What is the Ka of the weak…

A: Assuming the unknown weak acid is HA Hence the dissociation reaction of acid is  HA ------> H+ +…

Q: What is the Ka of a weak acid whose 0.10 M solution produces a pH of 2.38?

A:

Q: If the pH of a 0.55 M solution of acid is 5.4, what is the KA?

A:

Q: An unknown weak acid with a concentration of 0.450 M has a pH of 5.600. What is the Ka of the weak…

A: Calculate the hydrogen ion concentration as follows: [H+] = 10^(-pH) = 10^(-5.6) Let HX be the weak…

Q: 0.021 M solution of a weak acid (HA) has a pH of 4.19. What is the Ka of the acid?

A: Ka is acid dissociation constants of weak acid.  Weak acid dissociated feabily in aqueous solution

Q: An unknown weak acid with a concentration of 0.088 M has a pH of 1.80. What is the Ka of the weak…

A: Since it is not given whether the weak acid is monoprotic or polyprotic. Hence I'm assuming the acid…

Q: An unknown weak acid with a concentration of 0.058 M has a pH of 1.80. What is the Ka of the weak…

A: Assuming the weak acid is monoprotic acid HA. Hence the ionisation reaction of acid can be written…

Q: An unknown weak acid with a concentration of 0.070 M has a pH of 1.80. What is the Ka of the weak…

A: Weak acid dissociated feably in aqueous solutionpH is equal to negative logarithmic value of…

Q: An unknown weak acid with a concentration of 0.220 M has a pH of 5.600. What is the Ka of the weak…

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.