Sulfuric acid is a strong acid because 0 has low astion disecites completely in water O Monices in aus solution 02's very soluble in t D Question 4 The conjugate base of His OHO has no compatto 00 OHO' OCH

Q: Find the p H of a 0.439 M N a A solution. The salt completely dissociates intoNaus and Anus, N a is…

A: Pka= -logka Use formula of PH of salt which is mixture of strong base and weak acid. PH=9.32

Q: The pH of an aqueous solution of NaC₂H3O2 is (Hint: Split the compound apart into separate ions,…

A: The given compound: NaC2H3O2  The compound is a salt . When we dissolve the salt into aqueous…

Q: If CH3OONa is addddd to a solutiom of CH3COOH, i’d the pH of the acid going to increase or decrease

A: When the salt is added to the solution, then due to common ion effect, the solubility of an acid…

Q: In a solution, when the concentrations of a weak acid and its conjugate base are equal, A the system…

A: When we have weak acid and its conjugate base , it forms a buffer solution. (Acidic buffer) For…

Q: The pH of a 0.05 M acid solution is 1.4. What is [H] in that solution? If the K, for the acid is 3.3…

A: We know that pH is the negative logarithm of H+ ion concentration. that is  pH = – log[H+] ⇒[H+] =…

Q: In the laboratory a student measures the percent ionization of a 0.528 M solution of benzoic acid ,…

A:

Q: if 65ml of 0.25M naoh are combined with 76ml of 0.3M h2so4 .What is the pH if the solution is…

A: Given  Millimoles of H2SO4 = M x V = 0.3 x 76  = 22.8 mmol Millimoles of H+ ion = 2 x millimoles of…

Q: 3. Does u buffered solution always naintsiu a solution at pH ?7 Please explain. At what pH is huffer…

A: Buffer solutions: Buffer solution is defined as a solution that oppose changes in  while adding…

Q: unexciting monoprotic acid (HBob) is made by adding 0.133 mol of HBob inot 0.100 L of solution. The…

A: Given, Moles of acid = 0.133 mol Volume of acid = 0.100 L Molarity of Acid(C) = mole/volume      C =…

Q: a cetain juice sample has [H+] = 1.0*10-4(exponet)   a. what is the ph for this sample   b. what is…

A: Equations for pH, pOH calculation:

Q: A particular acid-base indicator has an acid ionization constant, KIn= 8.3E-11. What would be the…

A: In the acid base titration, the pKIn signifies the mid-point of the pH range in which a particular…

Q: 2) CalculatethepHduringthetitrationof15.00mLof0.1000MSr(OH)2with0.1000MHBr solution after 29.00 mLs…

A: Molarity of Sr(OH)2 = 0.1 M volume of Sr(OH)2 = 15 mLMolarity of HBr= 0.1 M volume of HBr = 29 mLBy…

Q: 1. At 25°C, a 50mL solution is found to contain 20% by mass acetic acid (CH3COOH). The density of…

A:

Q: In the laboratory, a general chemistry student measured the pH of a 0.576 M aqueous solution of…

A: pH = -log[H3O+]

Q: Choose the correct order based on the given criterion per line for comparative 1.5 M aqueous…

A: ->Acids has pH less than 7 , stronger acid has less pH. -> Base has pH greater than 7 ,…

Q: pH of 2.91 is prepared by dissolving I g. of benzoic ater. What is K of benzoic acid?

A: According to the question, a solution with a pH of 2.91 is prepared by dissolving 1 g. of benzoic…

Q: grai

A:

Q: E. Dry HCI HO(CH),CHO DHP HCrO, 7A 1) PhLi/EO 2) H"(aq)

A:

Q: 3. How many moles of sodium fluoride are produced when 0.789 moles of fluorine reacts with sodium…

A: Mole concept is a phenomenon used for the calculation of number of moles in a species. Number of…

Q: Consider the titration of 50.0 mL of 0.314 M weak base B (Kb = 7.5 x 106) with 0.340 M HNO3. What is…

A:

Q: What is the pH of an aqueous solution of KNO₂? (Hint: Split the compound apart into separate ions,…

A: If pH is less than 7 than solution is acidic in nature.   If pH value is more than 7  than solution…

Q: of 45 > Assuming equal concentrations, arrange these solutions by pH. Highest pH HCN(aq) HI(aq)…

A:

Q: An aqueous solution has An hydroxide ion concentration of IE-IM (10-'m). What is the hydronium ion…

A:

Q: A student dissolves a sample of a weak acid, HA, in 20.0 ml of H;O. The student then takes 5.6 mL of…

A: Given, Volume of water = 20.0 mL Volume of sample = 5.0 mL pH of final solution = 4.5

Q: ALL BEAICF 12 AN of 100 mL SOLUTION; HAve A QU EOUS 0.1M A: HN 03 B:HN O2 Ka = 7.2 X /0 CHNO;) = %3D

A: Since beaker A has acid HNO3 with concentration = 0.1 M  And beaker D has H2SO4 with concentration =…

Q: Lant values II A solution contains 0.262 M sodium nitrite and 0.297 M nitrous acid. The pH of this…

A:

Q: balamıd the Solution. Show each step involud in balaneng the reachon deanly. bedox reaction thaT…

A:

Q: Which of the following is NOT associated with buffered solutions? O Minimizing changes in pH O Le…

A: Buffer solution are used to maintain pH.

Q: What volume (in mL) of 9.2 M HCIO, would be required to make 500.0 mL of a solution with a pH of…

A: In a mono-protic strong acid solution H+ concentration is always same with its actual concentration…

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.