Question: 1 .HA is a weak acid. Its ionization constant, Ka, is 1.3 x 10-13. Calculate the pH of an aqueous solution where the initial concentration of NaA is 0.050 M. 2 . Place 0.112 mol of a weak acid, HA, in enough water to make 1.00 L of solution. The final pH of this solution is 1.29. Calculate the ionization constant, Ka, of HA. 3 . Place 0.648 mol of a weak acid, HA, and 13.1 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.76. Calculate the ionization constant, Ka, of HA. Please complete answers than rating helpful other wise un helpful

Q: The Ka for four acids are H₂CO3: 4.5 x 10-7, HCO₂H: 1.8 × 10-4, H3C,H,O,: 7.1 x 10-4, HCN: 6.2 x…

A:

Q: You have a buffer solution containing an acid, HA. The pKa of HA is 7.20 and its conjugate base is…

A: Here we are required to find the pH of the buffer solution.

Q: weak

A: We used the Hinderson equation for calculating the concentration of salt ( NaA ) and it's acid ( HA…

Q: Calculate the percent ionization of a 1.00 M solution of hydrocyanic acid, HCN.

A: According to Bartlby guidelines i solve only first question.You post  Second question  separately.

Q: The pyridinium ion (C5H4NH) is a weak acid (Ka = 5.60 x 10-6). Calculate the pH of a solution that…

A:

Q: Sulfurous acid, H2SO3, is a diprotic acid Ka1 = 1.3 × 10-2 and Ka2 = 6.3 × 10-8. The acid forms when…

A:

Q: An engineer wants to determine whether a certain pH meter is working correctly.  She uses the meter…

A: Given: A pH meter is used to measure pH of 14 neutral samples. Readings are as follows:7.01, 7.04,…

Q: HX is a weak acid: Ka = 5.52 × 10–7. Calculate the pH of a solution in which [HX] = 0.0501 M and…

A: Here HX is a weak acid. Given data, Ka =5.52×10-7 [HX]=0.0501 M and [X1-]=0.00845 M

Q: A weak acid, HA, has a K₁ = 7.76x10-3. What is the pH of a solution with [HA] = 0.236 M and [NaA] =…

A: The pH of a mixture of a weak acid (HA) with its conjugate base (A-) is calculated using the…

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.