what is the difference in balancing an equation in acidic soultion and basic solution? can I get a simple example of each?

Q: How to prepare the following for a titration procedure? 1. 20 mL of 2 M HCl 2. 20 mL of 0.05 M KOH…

A: Molarity - It is defined as moles of solvent dissolved per liters of solution. The molar mass  of  H…

Q: A. What is the pOH of the solution at the half equivalence point? B. What is the ionization…

A: Given data :  Unknown base  solution  = 10 ml .  Titrated with known concentrated HCl of molar…

Q: A solution contains 0.119 M ammonium chloride and 0.126 M ammonia. The pH of this solution is

A: The given data contains, Molarity of ammonium chloride = 0.119 M. Molarity of ammonia = 0.126 M pKb…

Q: A 0.667 M solution of a weak base has a pH of 10.80. What is the base hydrolysis constant, ?b, for…

A:

Q: A 0.135 M solution of a weak base has a pH of 11.23. Determine Kb for the base.

A: Weak base are those which do not dissociate completely in water. For base concentration depend on…

Q: What is the effect of the sprite/baking soda mixture on the acidity and basicity on a mixture?

A: The Chemical name of Baking Soda is Sodium Bicarbonate and has pH of 9. It is found in most of the…

Q: A solution contains 0.392 M NH¸I and 0.134 M ammonia. The pH of this solution is

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Q: A solution is prepared by diluting 20.0 mL of 0.0010 M HCl to a final volume of 2.00 liters. What…

A: Consider the given information is as follows; Volume of initial HCl solution V1= 20.0 mL = 0.02 L…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0106 M solution. The pH of the…

A:

Q: I am having a hard time determining when to use the Hasselbalch equation vs when to use other…

A: Answer: Henderson-Hasslebalch equation is used for the calculation of the pH of buffer solution. To…

Q: What is the pH of a 0.627 M weak base solution? The Kb of the weak base is 0.000066.

A: Given :- concentration of weak base solution = 0.627 M  Kb for weak base = 0.000066  To calculate :-…

Q: A solution containing 572.0mL of 0.6300MHCl is diluted to a volume of 1.000L. What is the pH of this…

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Q: You dissolve some BeF2 in water. Is the resulting solution acidic, basic or neutral?

A: The species which accepts the electron pair is known as Lewis acid The species which donates the…

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

A: The given equation is  (CH3)3NHBr -------> (CH3)3NH+  + Br-

Q: A solution containing 572.0mL of 0.6309 M HCl is diluted to a volume of 1.000 L. What is the pH of…

A: "pH" is utilized to analyze the quantity of [H+] ion in concentration term in any solution. It…

Q: A solution contains 0.305 M ammonium bromide and 5.90x10-2 M ammonia. The pH of this solution is

A: given :-  concentration of ammonium bromide = 0.305 M  concentration of ammonia = 5.90 × 10-2 M  To…

Q: Give a example of an acid base titration with the equation other than naoh and hcl

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Q: A solution contains 0.281 M ammonium bromide and 0.480 M ammonia. The pH of this solution is

A: Given data contains, Concentration of ammonium bromide is 0.281 M. Concentration of ammonia is 0.480…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0184 M solution. The pH of the…

A: Acids are the compounds which donate protons, H+ in the solution. Weak acids partially dissociate…

Q: Consider a HCI solution with a pH of 4.70. a) Calculate the concentration of HCl. b) Identify the…

A: pH is he negative logarithm of hydrogen ions. pH values can range from 0 to 14. pH is used to know…

Q: Which ions are present in all acid-base systems? Explain your answer using the Kw. How do you know…

A: An acid gives H+ and a base gives OH- ion in aqueous solution according to Arrehenius acid-base…

Q: A solution of an unknown chemical has a pH of 9. Is this solution acidic or basic?

A: Given A solution of an unknown chemical has a pH of 9.

Q: In the laboratory, a general chemistry student measured the pH of a 0.591 M aqueous solution of…

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

Q: A 0.825 M solution of a weak base has a pH of 11.83. What is the base hydrolysis constant, ?b, for…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: Which of the following titrations result in a basic solution at the equivalence point?

A: In this question, we will Identify which titration will produces basic Solution at equivalence…

Q: A solution has [H+] or [H3O+] = 4.7 ×10–3 M. The [OH–] in this solution is

A: We know that [ H+ ] [ OH- ] = 10-14  As [ H+ ] = 4.7 * 10-3

Q: Which of the following solutions will h

A: the solutions which resists change in pH by the addition of small amount of strong acid (or) base…

Q: Which solution would have the higher pH: 0.010 M HNO2 or 0.010 M HNO3? Explain.

A: pH of any solution is defined as negative logarithm of H3O+ or H+ concentration present in solution…

Q: The ph of 168 mL of a .556 M solution of unknown weak base is 12.96. what is the Kb of this base?

A: Volume of solution =168 mL Concentration of solution=0.556 M pH =12.96 Kb=?

Q: At the equivalence point of a weak base against HCl, the solution contains only that of the base,…

A: ITS FALSE AS TITRATION OF  WEAK BASE AND STRONG ACID SUCH AS HCL GIVES OVERALL ALL ACIDIC SOLUTION…

Q: A solution contains 0.145 M ammonium chloride and 0.108 M ammonia. The pH of this solution is

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Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0169 M solution. The pH of the…

A: Given : Concentration of monoprotic acid, HA (assuming it HA) = 0.0169 M And pH of solution = 2.56…

Q: : What is the K, value for this weak acid?

A:

Q: e Which of the following acids is weaker: HCIO, or HCIO,?

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

Q: A solution is prepared by mixing 0.2 moles of HCl into water until the final volume of the solution…

A: pH = -log[H3O+]  This formula is used to calculate to pH .

Q: The pH of a basic solution is 12.51. What is pOH?

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Q: Weak acid a Amphoteric b O Strong acid.c O me of the abovedO

A: Hydrazoic acid is also called as  Hydrogen azide or Azoimide.

Q: Calculate for the [H+] of an oxalic acid solution with a pH of 4.7. What is the pOH and [OH-] of the…

A: We have given that  pH = 4.7 We know that pH = -log[H+]  [H+] = 10-4.7         = 2.0×10-5

Q: What will be the pH value of the solution if we have added aqueous NH4Cl to a neutral solution and…

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Q: LESSON: Acid-Base Titration Answer the following question. 1. What can be done to remedy a sample…

A: In acid base titration we use unknown concentration of acid with known volume and titrate it with…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.74 M solution. The pH of the…

A: Let, HA be the monoprotic acid. Given, concentration of monoprotic acid, [HA] = 1.74 M     and, pH =…

Q: How many moles of conjugate base should be added to 315 mL of 0.45 M HLac to give a pH of 4.00?

A: pKa of HLac = 3.85  Moles of HLac = 0.45 x 0.315 = 0.14175 mol Let moles of conjugate base ( Lac- )…

Q: A solution contains 0.280 M ammonium iodide and 0.161 M ammonia. The pH of this solution is

A: Given: Ammonium iodide [NH4I]= 0.280 M Ammonia [NH3] = 0.161 M pH = ? The given solution is a buffer…

Q: If 1.0 mL of 0.4 M HCl was added to 40.0 mL of pure water, what would the resulting ΔpH of the…

A: Since moles of HCl taken = volume of HCl in L X molarity of HCl = 0.4 X 1 / 1000 = 0.0004 Since HCl…

Q: 2. What pH values are considered acidic? How about basic? 3. What is the color of a basic solution…

A: pH is a measure of how acidic/basic water is. The range goes from 0 - 14, with 7 being neutral. pHs…

Q: The pH of a basic solution is 12.71. What is [H⁺]?

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Q: Which one of the following 1.0 M solutions would have the highest pH?

A: A large Kb value indicates the high level of dissociation of a strong base. A lower pKb value…

Q: Write the reaction responsible for the solution being basic. Spectator ions do not need to be…

A: Nature of solution whether is acidic or basic depend on the net ionic equation

Q: A- Define the buffer solution, and then prove that the dilution has no effect on the PH of a…

A: As per the bartleby guidelines, am expert is allowed to answer one question at a time.  Please re…

Q: Why is it uncommon for diprotic and triprotic acids to completely dissociate in an aqueous solution?

A: An acid is one which donates a proton wheras a polyprotic acid donates protons. Polyprotic acid…

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.