Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50.

Q: What is the pH of a solution with hydronium ion concentration equal to 0.0046 M.

A: Given :- concentration of hydronium ion in solution = 0.0046 M  To be calculated :- pH of solution

Q: Which of the following solutions would be expected to have a pH of 7.00?

A:

Q: Calculate the pH and [OH'] of a 0.001 M solution of NaOH.

A: Given :- molar concentration of NaOH = 0.001 M  To calculate :- [OH-] and pH of the solution

Q: the concentration of OH- in a sample of seawater is 5.0 x 10-6 M. calculate the concentration of…

A: We have to predict the hydronium ion concentration.

Q: What is the pH of a 0.00100 M solution of NaOH?

A: Inorganic chemistry.

Q: Write equations that show NH3 as both a conjugate acid and a conjugate base.

A: Conjugate base is formed from acids, when a proton or hydrogen ion is removed. Conjugate acids are…

Q: A solution of sulfuric acid (H2SO4) has a concentration of 0.0075 M. Calculate the pH of this…

A: Given, Concentration of H2SO4 solution = [H2SO4] =  0.0075 M pH of the solution = ? Note:  Sulfuric…

Q: Calculate the pH of each solution at 25 °C and indicate whether the solution is acidic or basic.

A: At 25°C, the pH of a solution is given by: pH = -log[H3O+] Also, At 25°C, the pOH of a solution is…

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

A:

Q: If the pH of a solution is 9.0 determine its [-OH] concentrations.

A: pH is the negative logarithm of H+ ion concentration, which indicates the concentration of hydrogen…

Q: Calculate the pH of a 0.87 M methylamine solution.

A: pH of solution is defined as negative logarithm of hydrogen ions.

Q: Use this data to rank the following solutions in order of increasing pH. In other words, select a…

A: For salt of weak acid and strong base.          pH = 7+{pKa + log[Salt]}/2        And pH>7 For…

Q: If ammonia (NH3) acted as a strong base, what would be the pH of a 0.1 00 M solution of ammonia?…

A:

Q: What is the pH of a 0.00250 M aqueous solution of sulfuric acid?

A:

Q: Calculate the molarity of the HCL solution if 0.074 mol of KCL is dissolved in water to make 2000 mL…

A: Given: Number of moles of HCl = 0.074 moles Volume of the solution = 2000mL = 2L

Q: What is the pH of a 0.00350 M solution of NaOH?

A: To determine the pH of a 0.00350 M solution of NaOH

Q: What is the pH of a solution with hydroxide ion concentration

A: pH = - log[H+]    At 25° C [H+]  [OH-] = 10-14  Given that [OH-] = 0.0076 M [H+] (0.0076 M) =…

Q: Calculate the pH value of 0.5 M NaCl

A: There can be 4 type of combinations of salt:A salt formed when a strong acid combines with a strong…

Q: Calculate the pH NaOH to 2.0 L o

A:

Q: 0.05 moles of Sr(OH)2 is dissolved in enough water to from 0.25L of solution. What is the pH of the…

A: Given that,  moles of Sr(OH)2 = 0.05 mol Volume of Sr(OH)2 solution = 0.25 L Molarity of Sr(OH)2…

Q: What is the pH of a 0.00545 M solution of NaOH?

A: pH is mathematically expressed as: pH=-log[H+] where [H+] represents the molarity of H+.

Q: What is the [H3O+] concentration of a solution that has pH + 11.61, 7.156, 0.015

A:

Q: Enter your answer in the provided box. A solution is made by dissolving 18.7 g of HCI in enough…

A: Answer: -0.023

Q: If the pH of a solution is 1.50, what is the concentration of [H+]?

A: pH of a solution is 1.50 We have to find the  concentration of [H+] We know that  pH = - log [H+]

Q: How much NaOH (in grams) is needed to prepare 546 mL of solution with a pH of 10.00?

A: ANSWER IS :

Q: Calculate the pH of the following solutions.  1.50 g of NaOH in 50 mL of the aqueous solution

A: Given: The amount of sodium hydroxide present in 50 mL of water is 1.50 g.

Q: What is the pH of an aqueous solution with an OH- concentration of 0.00250 M?

A: Solution:- Given concentration of OH- = 0.00250 M  [OH-] = 0.00250 M  As we know, p(OH) = -…

Q: Calculate the pOH and pH of a 0.0045 M solution of NaOH.

A: concentration of NaOH solution is 0.0045 M  we have to find pH and pOH of solution  pH = -log[H+]…

Q: Calculate the pH value of 0.5 M NaOH

A: As NaOH is very strong electrolyte i.e base so it will dissociate completely  :…

Q: Calculate the pH of 0.0500 M aqueous solution of Methylamine.

A: Concentration of a solution can be measured in terms of molarity, molality and normality.

Q: If the solution concentration is 1.0 x 10-4 M HCl, then the pH value is equal to ______  and the…

A: pH is the negative logarithm of Hydrogen ion concentration. It is potential of Hydrogen ion…

Q: Write equations that show H2 PO4− acting both as an acid and as a base.

A: An acid is a substance that can donate a proton. Conjugate base is formed when an acid has donated a…

Q: Calculate the pH of a solution that has [OH-] = 1.0 * 10 -6 M

A:

Q: What is the pH of (a) a 0.028 M solution of NaOH

A: Given: Concentration of NaOH=0.028M To find: The pH of the solution

Q: What is the ph of a 0.00130 M solution of NaOH

A: Concentration of NaOH = 0.00130 M  pH of the solution of NaOH = ?

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

A:

Q: What is the pH of NaOH that has a concentration of 0.013 M?

A: NaOH is a strong base and dissociates completely as Na+ and OH- in solution. As it dissociates…

Q: Calculate the pH of a 0.74 M solution of NaOH.

A:

Q: Write the formula for the conjugate base of NH,".

A: Answer:- This question is answered by using the simple concept of writing the conjugate base of the…

Q: Calculate the pH of a 0.098 mol L–1 NaOH solution

A: The pH can be determined through the formula,  *pH + pOH = 14  *pOH = -log[OH-]

Q: Write the equation for dissolving Hydrochloric acid in water (include water). Identify base, acid,…

A: Strong acids are those which get completely dissociated in water. Some examples of strong acids are…

Q: Calculate the hydrogen-ion concentration and pH of 0.0350 M KOH.

A: KOH completely dissociate into  KOH ------>K +  + OH- At 25o C  Ionic product (K w )   of  water…

Q: Calculate the hydroxide ion concentration of a solution with a pH of 12.65.

A: Given :- pH of solution = 12.65  To calculate :- hydroxide ion concentration i.e. [OH-]

Q: solution

A: We will calculate H+

Q: Calculate the pH of the following acid or base: 2. 2.0x10 M NaOH

A: Given: [NaOH] = 2.0 x 10-4 M = [OH-] pOH = - log[OH-]          = - log (2.0 x 10-4 )         = 4 -…

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−][OH−], of 7.69×10−7 M.

A: Calculate the pOH of the solution,            pOH =- log [OH-]= - log (7.69 × 10-7)= 6.11

Q: Calculate the pH of a 0.00015 M NaOH solution. NaOH is a strong base and completely dissociates in…

A:

Q: What is the pH of a 0.00760 M solution of NaOH?

A: Given concentration of NaOH = 0.0076 M

Q: What is the hydrogen ion concentration, pH, and pOH of a solution with a hydroxide ion concentration…

A:

Q: Predict the given compound by writing: SA(For Strong Acid), SB(For Weak Base), WA(For Weak Acid),…

A: We have to predict the following given compound is stronge acid or weak acid as follows in step 2:

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.