What concentration of sodium hydroxide is needed to give an aqueous solution with a pOH of 4.600? Molarity of sodium hydroxide = M

Q: How many moles of H+ are present in 33.7ml of 0.124M HCL solution?

A: Given: 33.7 mL of 0.124 M HCl

Q: A 1.45 g sample of acetic acid , HC2H3O2 was burned in excess oxygen in a bomb calorimeter. The…

A: We have to predict the heat of combustion.

Q: What is the pOH of an aqueous solution of 3.77 x 10-2 M sodium hydroxide? pOH =

A:

Q: Calculate either [H,O] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.59 x 107…

A:

Q: What is the pOH of an aqueous solution of 0.138 M hydrochloric acid?

A: pOH is used to determine the concentration of hydroxide ion.

Q: What is the pOH of an aqueous solution of 4.45x10 M potassium hydroxide? РОН -

A: A strong base is one which is capable of complete ionization in aqueous solution. It produces a…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as an acid,…

A: As we know,  pH = - log [ H+ ]  & pOH = - log [ OH-]  where [ H+ ] & [ OH-]  are…

Q: An ionic compound if formed between the cation X+3 and the anion Y-2 What is the formula of this…

A: The numerical value of the two atoms' ion charges is crossed across when using the criss-cross…

Q: Would a 1.0 * 10-8M solution of HCl have pH 6>7, pH = 7, or pH <7?

A:

Q: Q14- A 0.100 M solution of the weak acid HA has a pH of 2.36. Calculate pK, for HA. 2.36 C) 1.66 B)…

A: Given: The pH of the weak acid, Ha = 2.36 The concentration of HA = 0.100 M We have to calculate the…

Q: What is the pOH of an aqueous solution at 25 degrees Celsius that contains 0.0009 M hydronium ion?

A: At 25 degree Celsius, [H+] [OH-] = 1 × 10^-14 pOH = -log(OH-)

Q: What is the concentration of OH in 0.64 M HNO3?

A:

Q: Buttercup acid is an organic compound that is a liquid at room temperature and is neutralized by…

A: Given : Mass of butyric acid = 0.215 g Concentration of NaOH solution = 0.150 M The reaction taking…

Q: The hydroxide ion concentration, [OH-], of an aqueous solution of 0.546 M hydroxylamine (a weak base…

A: Concentration of hydroxylamine = 0.546 MKb of hydroxylamine

Q: Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That…

A: pH is defined as negative logarithm of H3O+ ion concentration. pH = − log [H3O+]

Q: What is the concentration of chloride ions in a 0.125 M MgCl2 solution?

A: The concentration of chloride ions in a 0.125 M MgCl2 solution is to be calculated

Q: Calculate the volume of concentrated HCl 12.2 M needed to prepare a solution of 50ml 3.0 M HCl.

A:

Q: Calculate [OH−][OH−] given [H3O+][H3O+] in each aqueous solution [H3O+]=6.2×10^−4M?

A: Here we have concentration of  i.e. [H3O+]=6.2×10^−4M From this we can calculate pH first pH = - log…

Q: Calculate either [H3O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 1.29 × 10-7…

A:

Q: Calculate the sodium ion (Na+) concentration for a 0.665 M Na3PO4 solution. [Na+] = ? M

A: The reaction for Na3PO4 dissociation is, Na3PO4 ------>3 Na+ + PO43-

Q: pOH of 13.33   What is the Molarity of hydroxide ions in the solution?

A: Concentration and molarity are the same things. So we use the formula of poH and find out the…

Q: You have pure water at pH = 7. What do you predict the pH will be if you add one drop of strong acid…

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: What concentration of potassium hydroxide is needed to give an aqueous solution with a pOH of 2.470?…

A:

Q: What is the percent ionization of H₂NNH₂ in a solution with a concentration of a 0.580 M? (Kb = 1.3…

A:

Q: What concentration of potassium hydroxide is needed to give an aqueous solution with a pH of 10.170?…

A:

Q: Calculate either H,O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH¯] = 2.99 × 10'…

A: H3O+ is the hydronium ion which is the hydrated form of a proton. Its concentration in any solution…

Q: Calculate either [H,O*] or [OH¯] for each of the solutions at 25 °C. Solution A: [OH-] = 1.91 × 10-7…

A: for the given solutions, we need to calculate [H3O+] or [OH-]

Q: What concentration of potassium hydroxide is needed to give an aqueous solution with a pH of 11.270?…

A:

Q: What is the pH of an aqueous solution of 9.10×10-3 M nitric acid? pH =

A: Given concentration of nitric acid is 9.10×10-3 M. Relation between pH and concentration of…

Q: What is the pOH of an aqueous solution of 0.464 M hydrochloric acid?

A: The pH is defined as the negative logarithm of hydrogen ion concentration. The pH value more than 7…

Q: How much more H+ is in water at a pH of 3 when compared to a pH of 6?

A: The equation relating pH and concentration of H+ is given below.

Q: What is the concentration (molarity) of HClO in a solution that is 0.168 M LIClO at 25°C?

A: Weak acid are those which does not dissociate completely in aqueous solution and weak base are those…

Q: A particular solution has a [OH−1] = 9.82×10−5. Calculate the [H+1] for this solution

A:

Q: What is the pOH of an aqueous solution of 6.78x102 M potassium hydroxide? pOH =

A: The given data is as follows: The concentration of potassium hydroxide = 6.78×10-2 M The pOH of the…

Q: What concentration of barium hydroxide is needed to give an aqueous solution with a pH of 9.640?…

A:

Q: What is the concentration of sodium ions in 0.170 M Na₂HPO₄?

A:

Q: What concentration of barium hydroxide is needed to give an aqueous solution with a pOH of 1.720?

A: Since barium hydroxide is a strong base Hence it will dissociate completely as per the reaction…

Q: Calculate [OH−][OH−] given [H3O+][H3O+] in each aqueous solution [H3O+]=5.6×10^−12M

A:

Q: Which neutralization will produce more water? potassium hydroxide is reacted with phosphoric acid…

A: In a neutralization reaction, an acid and a base react quantitatively to form salt and water…

Q: What concentration of potassium hydroxide is needed to give an aqueous solution with a pH of 11.220?…

A: • The values provided in the question are:-       i) pH of KOH solution = 11.220      • We need to…

Q: An aqueous solution at 25 °C has a H₂O* concentration of 5. × 10 M. Calculate the OH concentration.…

A: Answer: In this question concentration of H3O+ ion is given to and we have to find out the…

Q: What is the pH of an aqueous solution of 2.37×10-2 M nitric acid? pH =

A: The important thing to keep in mind here is that nitric acid is a strong acid, which means that it…

Q: icmillan Learning Calculate either [H,O*] or [OH-] for each of the solutions at 25 °C. Solution A:…

A: At 25°C , H3O+×OH- =1×10-14 PH=-logH3O+ When PH of the solution is >7, then it is a basic…

Q: Calculate either [H3O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.15 x 10-7…

A: • [H3O+] × [OH-] = 1 × 10-14 • pH = -log[H3O+]

Q: What is the percent ionization of H₂NNH₂ in a solution with a concentration of a 0.660 M? (Kb = 1.3…

A: % ionization = 0.140%

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.