9. In `CH,OH 5. A buffer solution contains H2CO3 and HCO3, resulting in the equilibrium shown by the reaction belo According to this reaction and LeChatelier's principle, what happens when acid (H3O*) is removed from this buffer solution? H2CO3 + H20 HCO3 + H3O* a. More HCO3 is formed. b. More H20 is formed. C. More H2CO3 is formed d. Less HCO3 is formed. e. The reaction shifts to the left.

Q: Can you explain it step by step?

A: Given:pOH of the soft drink = 8.53 To find the concentration of [H3​O+] The pH of this drink is…

Q: Calculate the pH and pOH of each solution at 25 °C. a. [H30'] = 1.7 x 10M c. [H,O'] = 2.2 x 106M b.…

A: Given,

Q: Which of the following salts produces a neutral solution when dissolved in water?   a. NaClO 4…

A: NaOH + HClO4 ---> NaClO4 + H2O  SB          SA                Salt         Water HF      +   KOH…

Q: A solution with a pOH of 11.70 has an [H+] of a. 5.0 × 10−3 M.b. 3.2 × 10−4 M.c. 2.0 × 10−12 M. d.…

A: Given data, pOH of the solution =11.70

Q: 10. a. In a neutral solution, what is the concentration of H3O+? 1.0 x 10-7 M b. In a neutral…

A: 10. pH of a solution is the negative logarithm of hydronium ion concentration.

Q: Consider the following equilibrium: H3O*(aq) + HNO2(aq) + H2O (1) = NO2 (aq) In which direction (if…

A: Given reaction is  HNO2aq+H2Ol⇌H3O+aq+NO2−aq To find the direction of equilibrium shift if  (a) KNO2…

Q: The OH ion concentration of a blood sample is 2.6 x 10 M. What is the pH of the blood? blood O a.…

A: pH  =  - log [ H3O+ ]  pOH  =  - log [ OH- ]  pH  +  pOH   = 14

Q: g. Cooling the reaction down. Does the value of K change? How h. Adding NH3. Does the value of K…

A:

Q: 32. A lab technician is trying to determine the concentration of H₂SO4 in a car battery. She decides…

A: Titration is a laboratory technique used to determine the concentration of a solution by reacting it…

Q: What is the hydronium-ion concentration of a 0.30 M solution of HCN (K=4.9 × 10-10) at 25°C? a. 1.7…

A: The concentration of HCN is 0.30M The acid dissociation constant Ka is 4.9 × 10-10 Using the data we…

Q: 1) Consider HA (a strong acid) and HB (a strong base).  a. Write a balanced chemical reaction for…

A: Strong acid ionizes completely and increase H3O+ in aqueous solution. HA being a string acid it…

Q: a. Write the ionization reaction for HNO3(aq) b. Calculate the H+ concentration in 1.77M HNO3 c.…

A:

Q: An oxidizing agent will cause which of the following changes? A. PtO2 > PtO B. PtO3> PtO2 C. Pt(OH)2…

A: Oxidising agent adds oxygen or we can say that it oxidises the molecule. In option A , B it is…

Q: 3. The-product constant of water is 1.0 x 10-14 at 25 °C. At 40 °C, the constant is 3.8 x 10-¹4.…

A: Autoionization of water is basically a Bronsted-Lowry acid-base reaction in which water acts as an…

Q: What is one of the products formed when potassiurm hydroxide and hydrochloric acid are used in…

A:

Q: 2. Sulfur dioxide reacts with molecular oxygen to form sulfur trioxide: 2SO2(g) + O2(g) = 2SO³(g) At…

A:

Q: 10. What is the molecular geometry and molecular polarity for CH₂Cl, and SO, ²? 11. What do…

A: 10) ch2cl2= polar molecule because individual dipole do not cancel each other so there is net dipole…

Q: Express the equilibrium constant (K) for the chemical equations. (Note the physical states) A.…

A: Equilibrium constant is the ratio of the multiplication of concentration of all products having…

Q: what is the equation that best describes what happens H2S dissolves in water?

A: H2S is and acid and it behave like arhenius acid when dissolve in water. Arhenius acid - Those…

Q: /hy: eaction? are equilibrium arrows used in this reaction? What type of reagents that be used to…

A: This question have two questions, first is why we used Equilibrium arrow, and second is what type of…

Q: 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium,…

A: Given: Initial moles of HA = 0.030 moles Volume of container = 2.0 L Equilibrium concentration of HA…

Q: What is [H3O + ] in each of the following acid solutions? a. 0.20 M HNO3 (aq) b. 1.0 M H3PO4 (aq) c.…

A: We only give the answer up to 3 sub-parts. Please resubmit the question for the rest sub-parts.

Q: Identify the two “active species” in each of the following buffer systems. a. HF and LiF b.…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: Fill in the left side of this equilibrium constant equation for the reaction of dimethylamine…

A: Given that,Weak base = Equilibrium constant expression when dissolved in water = ?

Q: Calculate [H+] and pH in a solution in which lactic acid, HC3H5O3, is 0.250 M and the lactate ion,…

A: Concentration of lactic acid = 0.250 MIt is required to calculate pH and H+ when variable amounts of…

Q: H3CO OH 2 HCONH2

A: The carbonyl compound reacts formamide and results in the formation of an imine. The reaction takes…

Q: In a 1.2 M solution of HCIO4, a strong acid, [H30"]= and [OH ]: %3D O a.83 x 10-15 M; 1.0 x 10 14 M…

A: HClO4 is a strong acid and strong acid dissociates completely into an aqueous solution.

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.