Complete the balanced neutralization equation for the reaction below: NH4OH(aq)+H3PO4(aq)--->

Q: A solution contains 0.675 grams of ethylamine (C2H7N) per 100.00 mL of solution. Electrical…

A: Given data,Mass of ethylamine=0.675gVolume of solution=100mL=0.1LPercent conversion=98%

Q: Complete and balance the following neutralization equations. ____ NaOH (aq) + ____ HBr (aq)  ____…

A: Neutralization reaction is the reaction between an acid with a base, results in the formation of…

Q: Consider H3A a triprotic acid with Ka1 = 3.0 x 10-3, Ka2 = 5.6 x 108 and Ka3 = 8.1 x 10-13, %3D %3D…

A:

Q: Carbon dioxide in the atmosphere dissolves in raindrops toproduce carbonic acid (H2CO3), causing the…

A: To find the range of [H+] and [OH-] in the raindrops can be given by- Since, Product of the both…

Q: A diprotic acid has ka1= 4.3×10^-6 and ka2= 5.5×10^-9. What will be the pH of a 0.77 M solution of…

A: In this question, we want to determine the pH of the Solution of the acid.  You can see details…

Q: Which equation shows a weak acid in water? O LIOH(s) –-> Li* (aq) + OH(aq) O HF(aq) + H,0(1) CI…

A: Weak acid is an acid that dissociates weakly i. e. it forms very low concentration of H+ in the…

Q: A solution is made by dissolving 13.9 g of HONH:CIO3 in 500.0 mL of water. Does CIOS- have any…

A:

Q: Methylamine, CH3NH2, is a weak base.CH3NH2(aq) + H2O(ℓ) ⇄ CH3NH3+(aq) + OH−(aq)If the pH of a 0.065…

A: Given data contains, pH=11.70 Concentration is 0.065 M. The pOH is calculated as, The pOH is 2.30.

Q: A solution with a pH of 10.11 would be classified as basic A solution with a pOH of 13.54 would be…

A: Given 1. pH = 10.112. pOH = 13.543. [O-H(aq.)] = 3 × 10-2mol/L4. [H3O+(aq.)] = 8.3 × 10-11mol/L

Q: Identify HC2H3O2(aq)HC2H3O2(aq) as an acid or a base. Identify KOH(aq)KOH(aq) as an acid or a base

A: In simple words acid is a substance which donates H+ ion and accept electrons. Base is a substance…

Q: Solution A has pH of 3.20, solution B pH of 12.50, solution C a pH of 7.00, and solution D a pH of…

A:

Q: much

A: Volume 15 ml and pH = 1.5

Q: Arrange the following 0.10 M solutions in order of increasing acidity: (i) NH4NO3, (ii) NaNO3, (iii)…

A: Salt are produced by the reaction of an acid and a base. For example, The nature of salt solution…

Q: Use the following information to answer question 36. Trichloroacetic acid, CC13COOH(aq), is used in…

A: Acidic species after loosing proton form conjugate base. Amphiprotic species is species which can…

Q: Which of the following is a Brønsted-Lowry acid-base reaction? O…

A:

Q: In which one of the following reactions does an H2O molecule behave as a Lewis base?   A.  H2O(l) +…

A: On the basis of Lewis concept, acid-base behavior can be defined as follows: 1. Lewis acid: Those…

Q: CH₂COOH(aq) is classified as a # acid. The reaction equation with water utilizes which of the…

A: A weak acid is that acid which do not undergo complete dissociation in water.

Q: Which one of the following represents the ionization of phosphoric acid? O A) Mg(OH)2(s) -->…

A: Write ionisation reaction of phosphoric acid ?

Q: Which of the following salt solutions will be neutral? Nal, K2CO3, Cu3(PO4)2, KCI, Sr(N03)2 O a) Nal…

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Q: Calculate the hydronium ion concentration in an aqueous solution of 7.34×10-2 M ascorbic acid,…

A: The acid dissociation constant Ka represents the acidic strength of a solution. When the value of Ka…

Q: Calculate the volume of 0.650-M NaOH solution needed to completely neutralize 28.1 mL of a 0.760-M…

A: The neutralisation reaction taking place will be  2 NaOH + H2SO4 --------> Na2SO4 + 2 H2O hence…

Q: The AIDS drug zalcitabine (also known as ddC) is a weak base with a pk, of 9.8. What percentage of…

A: The given data: pKb of the drug = 9.8 The amount of drug present in solution = 565 mg/L. To…

Q: ive the definitions for the following scientific terms. a. Acid b. Base c. pH

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: aq 6. (1) Define pH in words. The strong acid HCI has a pH value of 1, use the following equation…

A: 6)  HCl(aq)  ➝ H+(aq) + Cl-(aq) i) Define pH = ? HCl is a strong acid. pH of the solution = 1…

Q: Name the following chemicals [hint: they are either acids or bases]: (a)  H2SO3(aq)          (b)…

A: Acids are those which donate H+ ion. Bases are those which accept H+ ion. All given compounds are…

Q: Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that pKal pKa2 pKa3 one molecule of the…

A:

Q: Identify the acid and base in the following reaction: HNO2 + KOH H2O+ KNO2

A: Given :-  HNO2 + KOH → H2O + KNO2  To identify :-  Acid and base in given reaction

Q: Calculate the pH of a 0.0644 M anilinium chloride solution. pH= Calculate the concentrations of…

A: Let us consider a ICE table below, HA = conjugate acid = 0.0644 M (anilinium chloride ) A- =…

Q: does H2SO4 act as a strong or weak acid in water

A:

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Interpretation: Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3×10-7 and Ka2 = 5.6 × 10-11.…

Q: Citric acid, which is present in citrus fruits, is a triprotic acid Is the concentration of citrate…

A: To find: Whether citrate ion is equal to, less than or greater than the H+ ion concentration.

Q: Calculate the concentration of HC6H₂O6 in an aqueous solution of 0.0337 M ascorbic acid, H₂C₂H₂O6…

A: Concentration of ascorbic acid (H2C6H6O6) = 0.0337 M  Concentration of HC6H6O6- = ?

Q: Calculate the concentration of CO32- in an aqueous solution of 0.174 M carbonic acid, H2CO3 (aq).…

A: Calculate the concentration of CO32- in an aqueous solution of 0.174 M carbonic acid, H2CO3

Q: 0.254M HNO3 [H+] [OH-] Ph POH

A: Given: Concentration of HNO3 = 0.254 M

Q: What are the products of the reaction between HNO3 (aq) and NaOH (aq)?

A: An acid is a substance that gives  ions in its solution whereas a basic substance gives  ions in its…

Q: Which of the following yields a basic solution when dissolved in water? I. NH3 II. Naz0 III. LIOH…

A: From the given chemicals, which one yields basic solution, when it was dissolved in water has to be…

Q: write out the stepwise ka reaction for the diprotic acid H2SO3

A: For a dissociation of acid (HA) in aqueous solution,

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: H2CO3 is weak diprotic acid so its pH is not directly calculated

Q: When the concentration of [HCO3-] is 61 mg/L at pH 7.0, express the concentration of CO2(aq) in mg/L…

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Q: How many mL of 0.45 M HCl(aq) are needed to neutralize a 149 mL solution of 1 M Ba(OH)2

A: Molarity is defined as number of moles of solute divide by volume of solution

Q: Identify the conjugate acid for each base. conjugate acid of HS¯: H,S conjugate acid of HPO; -:…

A: Since conjugate acid of any given base is formed by adding 1 H+ ion on the compound  hence the…

Q: Calculate the concentration of each species present in a 0.010-M solution of phthalic acid,…

A: Ka is defined as the equilibrium constant. It is the ratio of the concentration of products to the…

Q: What are the products of the reaction between nitric acid [HN03(aq)] and sodium hydroxide…

A: The reaction of a strong acid with a strong base gives salt and water. This type of reaction is…

Q: The daily output of stomach acid (gastric juice) is 1000 mL to 1400 mL. Prior to a meal, stomach…

A: pH of any acidic or basic solution is given by ----- pH = -log10H3O+ where [H3O+] is the…

Q: Of the following, ________ is a weak acid. A) HF B) HCl C) HBr D) HNO3 E) HClO4

A: Acidic strength of any acid is decided by the ability of acid to produce protons in the solution.…

Q: Identify KOH(aq) as an acid or a base.  Write a chemical equation showing how this is a base…

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Q: If the pH of a 0.0850 M solution of HBrO2 is 2.29, then what is the value for the acidity constant,…

A: pH = -log[H+] Relation between [H+], Ka and C of a weak acid solution: [H+] = (Ka x C)1/2

Q: At 25∘C, a pH of 3.2 corresponds to a pOH of:

A:

Q: Identify HC2H3O2(aq) as an acid or a base. Write a chemical equation showing how this is an acid…

A: Arrhenius acid-base theory: According to the Arrhenius theory, an acid is a substance that…

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.