A 10.0 ml of 2.0M sulfuric acid needs 12.5ml 25tds do of NaOH to neutralize it. compute for the ff. 19 Moles of acid 900 tips Moles of base POM 1/8

Q: 10. For which of the following is the K, value of the ionic com- pound the largest? The smallest?…

A: The solubility product of an ionic compound AxBy is given by: AxBy⇌xAy++yBx-Ksp=[Ay+]x[Bx-]y…

Q: which indicator C methyl in the red)will b 1owi o0ing (choose either pheno shang Stro ong acid CHc.…

A: Indicators such as phenolphalein and methyl orange is used during titration to identify the…

Q: The hydroxide ion concentration, [OH], of an aqueous solution of 0.555 M aniline (a weak base with…

A: Given, Concentration of aniline (C) = 0.555 M  Hydroxide ion concentration= [OH-] = ? Note:  Kb for…

Q: The pH of an aqueous solution of 0.170 M sodium acetate, NaCH3COO, is | (Assume that Ka (HCH3COO) =…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: A 0.10 mol/L solution of ammoia, NH3(aq) has a pOH of 2.89 at a certain Determine K₁ for ammonia at…

A:

Q: 0.2306m to in show the sol

A:

Q: How many mL of 0.185 M NaOH will be required to completely titrate 10.5 mL of 0.200 M H,SO,? (Hint:…

A: Molarity is defined as the amount of solute expressed in the number of moles present per liter of…

Q: Question 6:- What salts (acidic. basie . neutral)z a, Na, GOu b, NaCHal00 (baric) 3 Nall Is the…

A: Hi, we are supposed to answer one question. To get the remaining questions solved please mention the…

Q: The "concentration" of water is 55.5M. Calculate percent ionziation.

A:

Q: 4. What mass of HCI(g) must be dissolved in 1.50 Lof a NaOH solution having a pH of 11.176 to…

A:

Q: Calculate the pH of a solution made by mixing 25.00ml. of 0.1056M HCI with 13.23ml of 0.1138M NAOH…

A: The acid solution is the solution in which loss of proton takes place and the pH of the solution is…

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: H3PO4 (first dissociation is strong, second and third are weak) 7.52×10-3=x20.1-xx=H2PO4-=0.0239M

Q: HFag) HSO, (aq) F (aq) 7.

A: This is an example of acid base reaction.

Q: re insmucted to make 400 nod 22 soln to mztch the pt of the first and Li6 Mnimc acid. Whet volume of…

A:

Q: Use the References to access important values if needed The hydroxide ion concentration in an…

A: #Q.1: Given the hydroxide ion concentration, [OH-(aq)] = 0.054 M

Q: 3. Volume of NAOH at the equivalence point- 4. Half the volume of NaOH at the equivalence point---…

A: According to question, In question volume of NaOH is given and change in pH when NaOH is added to…

Q: Write the formula for the conjugate acid of each of the following. (Omit states-of-matter from your…

A: Solution - conjugate acid have one more H atom and one more positive charge so we will add one H…

Q: O Determine if the following salts are acidic basic or neutral. The following link has a list of…

A:

Q: Determine the Kb of this base. (Need to show all steps of calculation)

A: Given: It is given that,"A solution of a weak hypothetical base (B) was made. The pH of 0.185 Molar…

Q: A solution is 0.0500 M in NH.Cl and 0.0250 M in NH3. K. (NH,) = 5.70 x 10-10 Calculate the pH of…

A: A buffer is a solution that resists the change of pH upon the addition of a small amount of acid or…

Q: The Ka of the weak acid HSO4- (aq) is 1.2*10-2 Give the weak acid's conjugate base and calculate the…

A: The objective of the question is to identify the conjugate base of the weak acid HSO4- and calculate…

Q: D 121HHLH ← → https://www-awu.aleks.com/alekscgi/x/Isl.exe/10_u-IgNslkr7j8P3jH-IBMBkpcnaFu0F7UJ....…

A: Atoms are made up of subatomic particles called electrons, protons and neutrons. Protons are…

Q: a) 25.0 ml of 0.80M KCI + 35.0 ml of 0.40M KOH b) 20.0 ml of .20M HCI + 30.0 ml of 0.10M NaOH c)…

A:

Q: 8 01:17:17 The Ka for the weak acid HA is 6.53 x 10^-7. Calculate the Kb for conjugate base A at…

A: Given: The Ka for the weak acid HA = 6.53 × 10-7 We have to calculate the Kb for the conjugate base…

Q: Calculate the pH of a 0.0778 M aqueous solution of formic acid (HCOOH, K, = 1.8×10). pH =

A: The value of Ka for the formic acid is 1.8 × 10-4

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

A: pH = -log[H3O+]

Q: 1. Find the product of the [H3O*] and [OH] for all your solutions and record value on Table 2. oit…

A:

Q: Calculate the pH of ... .. 0.320 moles of H,SO, dissolved in 8.0 L of water.

A: Given moles of H2SO4 = 0.320  Volume of water = 8 L

Q: Titration of Carbonic Acid pH vs. Volume (ml) 12 10 10 50 Volume of Acidic Titrant Added (ml) 2. Hd

A: At 0 mL pH is dependent on the hydrolysis of Bronsted base [ Co3] 2- .

Q: . If BaCl2 completely dissolves in water, what is the ionic strength of a 0.0300 F solution of…

A:

Q: What is the number of moles of barium hydroxide in a 100 cm³ solution with a pH of 11 at 25 °C? (K =…

A: The question is based on the concept of pH of the solution.  It is defined as a negative logarithm…

Q: Calculate the pH of a 0.528 M aqueous solution of benzoic acid (C,H3COOH, K, = 6.3x10). %3D pH =

A: concentration of Benzoic acid (C6H5COOH) = 0.528 M   Ka of Benzoic acid = 6.3 x 10−5

Q: Q2} In the standardization of NaOH with 0.243 g of H,C,0,.2H,0 required 39.82 ml of 0.09M of the…

A: Use neutralisation equation  Mole× nfactor= M1V1(litre)

Q: Bellringer 29 - pH Calculations Which of the following aqueous solutions will have a pH that is…

A: Weak acid would have significantly different pH than that of strong acids.

Q: Calculate the pH of a solution that is (This problem requires values in your textbook's specific use…

A:

Q: Utilize the following normal values to determine the primary acid-base imbalance and compensation…

A: Normal Values pH = 7.35-7.45 pCO2 = 35-45 mmHg [HCO3-] = 22-26 mEq/L

Q: 2) The PH of asolution of aweak ronoprotic ucid (HA) is 2.85 what is the Ka of the acid ? Ans.: 2*10

A: Given ,  Concentration of weak mono protic acid ( C ) = 0.1 M pH of the weak acid = 2.85 Acid…

Q: 10. Which of the following chemical equations is an acid-base reaction? a. 2 HCl(aq) + Zn(s) → H2(g)…

A: Explanation to the correct answer is given below.

Q: A phase diagram for elemental carbon is shown below. How many triple points are present? 10 Diamond…

A: ->Triple point is point in phase diagram at which tree phases are in equilibrium.That is three…

Q: pH

A:

Q: A weak base solution is 0.20 M and is 2.5 % ionized. Calculate Kb.

A:

Q: moles of unknown acid equal moles of NaOH at the second equivalence point?

A: We need to examine conditions at second equivalence point.

Q: Calculate the pH of the solution that results when mixing 20mL of .2M HCl with 25mL of a.) distilled…

A: NOTE:  “Since you have posted a question with multiple sub-parts, we will solve first three subparts…

Q: In this experiment which is the acid and which is the base: 25.00 ml of 0.500 M HCl neutralized…

A:

Q: 0.150 M Express your answer using two significant figures. Submit Request Answer Part D 4.50x10-2 M…

A: The Question is based on the concept of equilibrium. we have to calculate percentage dissociation…

Q: A solution contains0.023Macetic acid and0.0.018Msodium acetate. The Ka for acetic acid is1.8×10−5.…

A: Molarity of acetic acid = 0.023 M Molarity of sodium acetate = 0.018 M Ka = 1.8 ×10-5

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.