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 of H:A?

Q: Calculate the pH of the solution.  Assume 1.0 L of solution. You must identify the type of solution…

A: HClO is a weak acid and RbOH is a strong base. Acid and base react to form salt and water. HClO0.250…

Q: The relative acidity of an aqueous solution is measured by the H+ ion concentration. pH = – log(H+)…

A: We know that PH=−log(H3​O+)[H3​O+]=10−PH[H3​O+]=10−3.5=0.00031622776601=3.162×10−4 M hence 1st…

Q: Carbon dioxide in the atmosphere dissolves in raindrops toproduce carbonic acid (H2CO3), causing the…

A: To find the range of [H+] and [OH-] in the raindrops can be given by- Since, Product of the both…

Q: The acid dissociation constant K of alloxanic acid (HCH₂N₂O5) is 2.24 × 10¯7. a Calculate the pH of…

A: Information of question

Q: water has a hydroxide ion concentration of 2.0 x 10-6 M. What is the pH of seawater?

A:

Q: What is the concentration of H+ ions

A: Given :- pH = 4.2  To calculate :- concentration of H+ ions   pH = -log[H+]

Q: A typical aspirin tablet contains 328 mg acetylsalicylic acid (HC,H;O,). Calculate the pH of a…

A: Given, Mass of one aspirin tablet = 328 mg So, mass of two tablet = 2×328 = 656 mg=0.656 g Final…

Q: Naturally occurring rainwater is acidic due to the presence of carbonic acid, H2CO3, produced when…

A: The problem is asking us to calculate the pH of rainwater given the concentration of carbonic acid…

Q: Given the weak acid, boric acid (H3BO3), calculate the pH and pOH of a 4M boric acid solution. Ka =…

A:

Q: Determine the pH of a 0.21 M solution of pyridinium nitrate (C5H5NHNO3) at 25°C. [Pyridinium nitrate…

A: To calculate pH , we need to calculate the concentration of hydronium ion given by pyridinium ion on…

Q: The pH of vinegar is about 2.5. Calculate the [H3O+] for vinegar.Calculate the [OH−] for…

A: The objective of the question is to calculate the concentration of hydronium ions [H3O+], hydroxide…

Q: Determine the pH of a 0.13 M solution of pyridinium nitrate (C5H5NHNO3) at 25°C. [Pyridinium nitrate…

A: Determine the pH of a 0.13 M solution of pyridinium nitrate

Q: * pH of a Strong Acid, a Weak Acid The pH of a solution is the negative logarithm of the molar…

A: Ph of given solution= 1.

Q: Calculate the pH and the pOH of these solutions:     (a) 0.257 M HBr pH =   pOH =     (b) 0.332 M…

A: Since you have posted a question with multiple sub-parts, we will solve first two subparts for you.…

Q: An aqueous solution at 25 °C has a pOH of 13.7. Calculate the pH. Be sure your answer has the…

A:

Q: What molar concentration of hydrazine, N2H4 (Kb = 1.7 x 10^-6) yields a solution with a pH of10.46?

A: The objective of this question is to find the molar concentration of hydrazine, N2H4 that yields a…

Q: Determine the pH of a 0.18 M solution of pyridinium nitrate (C5H5NHNO3) at 25 ° C. [Pyridinium…

A: Given,Molarity of pyridinium nitrate (C5H5NHNO3)  = 0.18 MKb = 1.7 × 10−9The value of Ka can be…

Q: he pH of a solution with [H+] = 1 x 10-9 M ?

A: The pH of a solution can be calculated using the formula given as,

Q: Calculate the pH of the solution and indicate whether each solution is acidic, basic, or neutral.…

A: Given: [H3O+]=1.97×10-4 To find: pH value and solution is acidic, basic or neutral. Solution: pH…

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H3O+], of 5.60 × 10-4 M. pH…

A: Hydronium ion concentration [H3O+] = 5.60 × 10-4 M. pH of the solution = ?

Q: Calculate the pH and [S2−] in a 0.10-M H2S solution. Assume ka1= 1.0 × 10−7; ka2= 1.0 × 10−19.

A: Answer:- This question is answered by using the simple concept of calculation of pH of a weak acid…

Q: Calculate the pH of an aqueous solution that is ( Ka(HCN) = 6.20 × 10 10-10) a. 0.870 M in HCN. pH =…

A: We know that  HCN is a weak acid it doesn't dissociate completely. The dissociation reaction will be…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.20 M solution…

A: Reactions- H₂A + H2O ↔HA-  + H3O+  Ka1 = 3.4 × 10⁻⁴ HA- + H2O ↔ A2- + H3O+  Ka2 = 6.7 × 10⁻⁹ Ka1…

Q: What is the pH of a 0.40 M solution of benzoic acid, C6H5COOH? (The Ka value for benzoic acid is…

A: given :- concentration of benzoic acid = 0.40 M  Ka for benzoic acid = 6.3 × 10-5  To calculate :-…

Q: 11. Identify the acid and the base that are reactants in each equation; identify the conjugate base…

A:

Q: What is the pH of a 0.177 M diprotic acid solution (H2A)? Ka1 = 4.3 x 10-5 and Ka2 = 2.8 x 10-9.

A: The general equation for the dissociation of a diprotic acid (H2A) can be represented as follows:…

Q: Calculate the pH of a 0.0307 M aqueous solution of nitrous acid (HNO₂, K₂ = 4.5×10-4). pH =

A: The question is based on the concept of pH of the solution.  It is defined as a negative logarithm…

Q: Ka for phenol (a weak acid), C6H5OH, is 1.00 × 10-¹⁰. Ka for acetylsalicylic acid (aspirin),…

A:

Q: Calculate the [OH−] and the pH of a solution with an [H+]=5.3×10−12 M at 25 °C.

A:

Q: What is the pH of a solution that has an H+ concentration of                        (a) 1.75 × 10 –5…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

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: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Given : Concentration of H2CO3 = 0.33 M Ka1 of H2CO3 = 4.3 X 10-7  And Ka2 of H2CO3 = 5.6 X 10-11…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Interpretation: Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3×10-7 and Ka2 = 5.6 × 10-11.…

Q: What is the pH of a 0.320 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: Ca(NO2)2 is a salt of weak acid HNO2 and strong base Ca(OH)2.  CaNO22 (aq) → Ca2+   (aq) + 2NO2-…

Q: What is the pH of a 0.190 M  solution of sulfurous acid? Given: Ka1 = 1.70×10–2, Ka2 = 6.20×10–8

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.