If the pH of two acids, X and Y, are pH 1 and pH 2 respectively, which of the following is true? IX and Y could be strong or weak acids II The concentration of [H] ions in X is higher than in Y III Acid X is stronger than acid Y

Q: What is the difference between a strong acid and a weak acid? Strong acids completely dissociate in…

A: Strong acids are substances that completely dissociate into ions when dissolved in water, breaking…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: The salt given is KC₃H₅O₃ Hence the ions present in it are K+ and C₃H₅O₃-

Q: Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral. compound…

A: If a salt is produced by the reaction of a strong acid and a strong base, then the aqueous solution…

Q: You measured the pH of a 0.01M NaOH solution (strong base) and it was 13.0. The, you diluted this…

A: pH is a graph that uses a logarithmic scale in which 7 is neutral, lower values are more acidic and…

Q: CH3COO-  (aq)    +   H+ (aq)   ⇔  CH3COOH  (aq), is an example of ________.     Bronsted base…

A: Acid base concept is given by Bronsted as well as Arrhenius . Arrhenius acid is that which…

Q: 1. Write the chemical reactions for both a weak acid and a strong acid. weak acid (HA) strong acid…

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Q: Consider two solutions: solution X has a pH of 5; solution Y has a pH of 7. From this information,…

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Q: The pH of this solution is _____ .

A: pH + pOH = 14.0  pH = -log[H3O+]  [H3O+] = 10-pH

Q: At a concentration of 1 M, the weak acid HNO2 is 2% ionized, and the pH of the solution is 1.7.…

A: Le-Chatlier's principle is used to govern the shift of equilibrium on introduction of additional…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 0.036 M. The hydronium ion…

A: The relation between all these terms ;  [OH-] = 0.036 M  [H3O+] [OH-] = Kw where Kw =1.0× 10-14   pH…

Q: Which of these solutions has the lowest pH? Rank these solutions: 0.10 M HIO, 0.10 M H2SO4, 0.10 M…

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Q: The pH of an aqueous solution at 25°C was found to be 3.10. The pOH of this solution is _____.…

A: pH = -log [H+] [H+] = 10-pH pOH = -log [OH-] [OH-] = 10-pOH pH + pOH = 14

Q: Calculate the [H+] and pH of pure water.

A: Kw of water at room temperature is 10-14.

Q: You measured the pH of a 0.01M HCI solution (strong acid) and a 0.01M CH3COOH solution (weak acid).…

A: We know that is strong acid have almost 100% dissociation of hydronium ion and weak acid have nearly…

Q: What are the hydronium and hydroxide ion concentrations in a solution whose pH is 7.95? [H*]. [OH-]-

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Q: Which of the three lines represents the effect of concentration on the percent ionization of a weak…

A: The percent ionization of an acid is the ratio of the concentration of ionized acid to the initial…

Q: Identify the weak monoprotic acid. Group of answer choices H2CO3 NaBr HF HNO3 LiOH

A:

Q: Which statement is correct?     The pH increases as the weak acid becomes diluted.     Unable to…

A: An acid which does not dissociate completely in aqueous solution is known as weak acid. Weak acids…

Q: ľ The pH found to The hydr The hyd.

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Q: Question 3 A student is given a concentrated solution that is supposed to contain vinegar, a weak…

A: A weak acid will not be completely dissociated in a solution. However, a strong acid will be…

Q: What is the concentration of hydroxide ion in a solution with a pH of 3.767?

A: pH of a solution is determined from the concentration of H+ ion in solution.  Now, pH = -log[H+]…

Q: If a solution has a concentration of hydronium ions less than 1.0 x 10-12 M would it be considered…

A: On the basis of pH value we can say whether the solution is acidic or basic. Firstly we need to…

Q: Which has a higher pH? 0.10 M of a strong acid 0.10 M of a weak acid

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: You find a very dilute solution of a very weak acid. Which of the following is true of the [H+]…

A: The question is asking about the concentration of hydrogen ions [H+] in a very dilute solution of 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.