For H2CO3, Ka1 = 4.3 × 10–7, Ka2 = 4.7 × 10–11. What is the pH of a 0.36 M solution of carbonic acid?

Q: The concentration of the hydrogen ions in an aqueous solution is 1.7 x 10-11. Determine the pH. Use…

A: Given [H+] = 1.7*10-11

Q: For H2CO3, Ka1 = 4.3 × 10–7, Ka2 = 4.7 × 10–11. What is the pH of a 0.36 M solution of carbonic…

A: We have to predict the pH of 0.36 M of carbonic acid .

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

A:

Q: Calculate the hydronium ion concentration, [H3O+][H3⁢O+], for a solution with a pH of 5.61

A: • The values provided in the question are:-      i) pH of a solution = 5.61    • We need to…

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: Consider a 1M solution that is prepared using the salt NH4NO3. The pKb of ammonia is 4.7 and the pKa…

A: The objective of the question is to determine which statements are accurate about the contents of a…

Q: The pH of a solution is 2.45. What is the molar concentration of hydronium ions in the solution?…

A: We have given that  pH = 2.45  [H3O+] = ?

Q: Calculate pH of a 0.1 M solution of AlCl3.

A:

Q: Is H2Cr2O2 an acid, base, or neutral? please justify your answer with an equation showing its…

A: The question is based on the concept of chemical substances  we need to identify the nature of the…

Q: Calculate the pH of 0.0037M solution of H2CO, given that K,1- 4.3 x 10 and Kz = 5.6 x 1011

A:

Q: The hydrogen ion concentration of a fruit juice is 3.3 x 10-2 M. What is the pH of the juice? Is it…

A: Given, [H+] = 3.3 x 10-2 M  PH is defined as negative logarithm of concentration of hydronium ion.

Q: What will be the pH of a solution containing 0.200 M NaH2PO4 and 0.200 M Na2HPO4? Ka(NaH2PO4) = 6.2…

A: Given,  Molar concentration of weak acid, NaH2PO4 or H2PO4- = [H2PO4-] = 0.200 M Molar concentration…

Q: Calculate the pH of a 0.350M aqueous solution of NH3 , The Kb of NH3 is 1.77 x 10-5

A: Given: The concentration of aqueous NH3=0.350M

Q: Ammonia is a weak base that is a household cleaner and has a Kb =1.8 x 10-5. What is the pH of a 3.0…

A: Given: Kb =1.8 x 10-5Concentration = 3.0 M pH = ?

Q: Calculate the pH of a 0.591 M aqueous solution of benzoic acid (CH₂COOH, K₂ = 6.3x10-5). pH =

A: Here,concentration of benzoic acid = 0.591 MKa = 6.3×10-5We have to find out pH.. Herw first we need…

Q: Phthalic acid (H₂CH₂O₂) is a diprotic acid with Kal = 1.12 x 10-3 and K₁2 = 3.90 x 10-6. Determine…

A: Given : acid is diprotic

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: What is the pH of a 0.138 M solution of H2SO4 (sulfuric acid)?

A: We will use formula of pH

Q: Calculate the pH of a 8.3 x 10-3-M solution of H2SO4 (K, = 1.2 x 10-2). %3D pH =

A: The given acid is H2SO4. It dissociates in solution to give two moles of H+ ions. The given…

Q: What is the pH of a 0.20 M solution of CH3NH3NO3 at 25 °C? At this temperature, the K₁ for CH3NH2 is…

A: Given:Given is a solution of CH3NH3NO3Concentration of solution = Temperature = 25oCThe pH of a…

Q: If the Ka for Al3+ is 1.00x10-5, then what is the pH of 0.250M Al(NO3)3?

A: Step 1: Step 2: Step 3: Step 4:

Q: 3. For the following Lewis acid-base reaction, identify the acid, the base, and the new covalent…

A:

Q: Calculate the pH of a 2.0 x 10–3 M solution of pyridine (C5H5N). Kb = 1.7 x 10–9

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

Q: What is the pH of a 0.20M solution of nitrous acid? Ka= 4.5x10^-4.

A:

Q: Calculate the pH at 25 °C of a 0.23M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

A:

Q: The pH of a fruit juice is 3.8. Find the hydronium ion​ concentration, H3O+​, of the juice. Use the…

A: The pH of the solution is a quantitative measure of the acidity or basicity of aqueous or other…

Q: What is the pH of a 0.950 M solution of Na2HPO4? H3PO4 is a weak polyprotic acid with Ka1 =…

A: The objective of this question is to calculate the pH of a 0.950 M solution of Na2HPO4. The compound…

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: The concept used over here is-Weak acid HA does not dissociate entirely, so it remains in the water.…

Q: Strawberries have a pH of 3.90. What is the [H3O+] and [OH-] of strawberries?

A:

Q: What is the pH of a 0.320 M solution of HC₂H₃O₂ (Ka = 1.8 × 10⁻⁵)?

A: Using the concept of the ICE table, we will calculate the equilibrium concentration of H+. Then we…

Q: What is the hydronium ion concentration [H3O+] of sea water which has a pH of 8?

A:

Q: The barium oxide is a strong electrolye:  BaO(s) + H2O(l) → Ba2+(aq) + 2 OH−(aq). What is the pH…

A:

Q: The Kb of hydrazine is 9.1 x 10-7. If 3.12 x 10-3 mol of hydrazine is added to water to make up…

A: Hydrazine (N2H4) is a weak base Concentration of hydrazine is calculated as follows,

Q: The acidity of a solution is measured by its pH. If H+ represents the concentration of hydrogen ions…

A: Given that :  pH of solution B = 3.4  using pH = -log[H+]  [H+] = 10-pH = 10-3.4 = 3.98 × 10-4 M So,…

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.