The equation shows reactants to a neutralization Which describes what will happen to the H+ when these reaction. reactants form products? Ca2+ + OH + H* + NO; O H* binds with NO; to make a salt. H* binds with Ca2* to make an acid. O Ht binds with OH to make water. O H* binds with Ca2+ to make a base.

Q: Calculate the [OH−] and the pH of a solution with an [H+]=6.3×10−10 M at 25 °C. [OH−]=     M pH=…

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Q: In the following equation, identify the acids, bases, and conjugate pairs. NH4+ CN NH3 + HCN (a)…

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Q: Macmillan Learning Calculate either [H₂O+] or [OH-] for each of the solutions at 25 °C. Solution A:…

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Q: Ka for nitrous acid, HNO2, is 4.50 × 10-4. Ka for hydrofluoric acid, HF, is 7.20 × 10-4. Ka for…

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Q: 1 point Each value represents a different aqueous solution at 25 °C. Classify each solution as an…

A: Answer:- This question is answered by using the simple concept of determination of nature of the…

Q: Complete the table. List the chemical formula of each species present at concentrations greater than…

A: From given  Chemical formula for each species is given when concentration greater than 10-6 mol /L

Q: In an aqueous solution, if H* increases then OH decreases. True O False

A: The question is based on the concept of equilibrium. ionic product of water is given as product of…

Q: Determine the [OH-]. pH, and pOH of a solution with a [H*] of 0.014 M at 25 °C. [OH-] = M pH = POH =…

A: At 25∘C,             Kw = OH-H+ = 1 × 10-14             pH = -logH+             pOH = -logOH-…

Q: H,PO4 is both a weak acid and a weak base

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

A: Strong Acids are the compounds which dissociates completely and give H3O+ ion in water. HA + H2O →…

Q: CH3CH2NH2 is a weak base, and HCl is a strong acid. One mole of the salt, CH3CH2NH3+Cl–, is added to…

A: This reaction is a acid base type reaction.

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.