What would the pH be at the equivalence point when citric acid is neutralized with sodium hydroxide?  Less than 0 Less than 7 Approximately equal to 7 Greater than 7 Greater than 14

Q: draw the strcture for ethonic acid

A: The objective of the question is to draw the structure of ethanoic acid.

Q: Calculate the percentage ionization of acetic acid in solutions having concentrations of 4.0 M, 0.40…

A: Acetic acid is a weak acid with the acid dissociation constant, Ka =1.76×10-5

Q: Place each compound into the appropriate category, based on how the compounds behave in water.…

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Q: Choose the correct left-to-right sequence of Bronsted-Lowry acid-base names for the left-to-right…

A: Third option. Acid, base, conjugate base, conjugate acid

Q: Based on the graph, how do know when the concentration of futylamine is equal to the concentration…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: HC4C3N2O3

A: Dear student I have given answer to your question in the image format.

Q: Addition of HCI to a buffer solution containing HC₂H3O2 and NaC₂H₂O₂ causes the pH to slightly…

A: When strong acid is added to buffer solution then it reacts with conjugate base of weak acid. In…

Q: A 0.100 M solution of NH4NO3 has a pH that is More information is needed Equal to 7 More than 7 Less…

A: pH of a solution can be figure out by considering the composition of salt.

Q: Which salt produces a basic solution when dissolved in water? O NANO3 O NaF O NH4CI O FeCl3

A: Answer:- This question is answered by using the simple concept of formation of salts. The salt…

Q: What is the OH- concentration of a 3.4 x10-6 MH3O+ solution scientific notation.   ____________ x…

A: [H3O+] [OH-] = 10-14

Q: Question 13 The pH of a 1.0 M benzoic acid solution i The % ionization in this situation is [Sel…

A: Given -> Molarity of benzoic acid = 1.0 M

Q: Match each solution with the correct description…

A: Given: To match the following: 1. dilute weak acid  18 M sulfuric acid 2. dilute strong base…

Q: In the following solutions, what is the change in hydrogen ion concentration? (how many times more…

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Q: Variation in the pH of certain lakes occurs sometimes over a 24-hour period. What might control lake…

A: The pH is known as the power of hydrogen in an aqueous solution. Acidic solutions have low pH…

Q: 2. Do you expect the equivalence point to be below a pH of 7, equal to a pH of 7, or above a pH of…

A: Equivalence point is that stage of titration at which amount of titrant added is enough to…

Q: When ammonia gas dissolves in water it acts as __________. an Arrhenius acid…

A: According to Bronsted lowry concept of acid and bases. The substance that donates the H+ ions in an…

Q: What is the concentration of Cl in the solution 0.25 M AlCl3

A: AlCl3 (aq) ------> Al3+ (aq) + 3Cl3- (aq)

Q: The pH value of an acid sometimes is unrelated to its dissociation constant, true or false? Select…

A: Statement : The pH value of an acid sometimes is unrelated to its dissociation constant. Assuming an…

Q: Draw pH vs titrant volume graphs for: I.A strong acid versus a strong baseii. A strong acid versus a…

A: A titration curve is a graph of volume of added base (or acid) vs. pH for a titration.The titration…

Q: What will happen to arsine as the pH is raised from 2 to 12?

A: Given is the Pourbouix diagram for As species.

Q: Indicate whether each of the following compounds will gave an acidic, basic or neutral solution when…

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Q: Can you explain how to find the equivalence point please

A: A graph based question about equivalence point concept, which is to be accomplished.

Q: If the K₂ of a weak acid is 1.6 x 10-8, the K, of its conjugate base partner must be which of the…

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Q: What is the concentration of hydrogen ion in a solution with a pH of 5?     1×1051×105 M 1 times 10…

A:

Q: 11) Do you expect NaCHO3 ( OR "N" a CHO3) to be acidic, neutral, or basic when dissolved in pure…

A: NaHCO3 commonly known as Sodium Bicarbonate or Baking Soda is Basic in Nature.

Q: If a base is added to an ester, what will happen? The ester will donate an acidic proton to the base…

A: In this question, what happened if base added to an ester compound.  You can see the details…

Q: Which acid ionization constant would indicate the weakest acid? Group of answer choices 3.5 x 10–4…

A: In any aqueous solution, strong acids tend to get ionized in greater extent. Whereas weak acids get…

Q: Which of the following is true if the hydrogen ion concentration of a solution increases? pH…

A: pH is quantitative measure of the acidity or basicity of aqueous or other liquid solutions. The pH…

Q: For a buffered solution consisting of   H2CO3 and HCO31-, which part of the buffer is used and which…

A:

Q: Which of the following is true about the pH scale? Group of answer choices A pH of 4 has a greater…

A: pH of any solution is given by  pH = -log[H+ ] = 14 + log[OH- ] where [OH- ] = concentration of OH-…

Q: salts? 1. LizC204 2. LİCIO 3. LICIO4 4. Li¿CO3 5. LiBr

A: 1. Li2C2O4 =  BASIC (salt of a weak acid and a strong base) Li2C2O4---> 2Li^+(aq) + C2O4^2-(aq)…

Q: The question is based on Vinegar Titration w/ NaOH  Before the endpoint, the solutions is: Basic or…

A: Given: Titration of vinegar with NaOH.

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.