10.0g of NaF is dissolved in water to make a total volume of 10.0L. Determine the pH of the solution. Ka=6.8X10-4

Q: Calculate pH and percent dissociation of 0.10 M HC6H5O (Ka=1.3x10-10)

A: Given information: 0.10 M C6H5OH Ka=1.3x10-10

Q: 0.35 g of hydrogen chloride (HCl) is dissolved in water to make 8.0 L  of solution. What is the pH…

A: Ph = -log (H+)

Q: Determine the pH of a solution that is 0.0075 M HC₄H₇O₂ and 0.085 M NaC₄H₇O₂. The value of Ka for…

A: Given, the concentration of HC4H7O2 =0.0075 Mconcentration of NaC4H7O2 =0.085 Mthe acid dissociation…

Q: Calculate the pH of a solution with a hydrogen ion concentration of 4.5×10^-6 M.

A: Given that, in a solution, the hydrogen ion concentration is [H+] = 4.5×10-6 M. We have to calculate…

Q: If one mole of Ba(OH)2 is added to enough water to make 10 liters of solution, the pH of the…

A:

Q: A solution is made by dissolving 30.1 g of Ba(NO,), in 500.0 mL of water. Using Kb(NO,) = 2.2 x…

A: The given salt Ba(NO2)2 on hydrolysis gives a mixture of strong base, Ba(OH)2 and a weak acid, HNO2.…

Q: Calculate the pH of each of the following strong acid solutions:(a) 8.5 x 10-3M HBr, (b) 1.52 g of…

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: Calculate the pH of a 0.50 M solution of oxalic acid, H2C2O4, given that (at the same temperature):…

A:

Q: solution

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Determine the pH of a solution that results when 15.0 mL of 2.00 mol/L NaOH is added to 25.0 mL…

A: This question belong to ionic equilibrium. pH calculation of mixture of strong acid and strong base.…

Q: Suppose you prepare a solution that consists of 34.00 mL of 1.0 M ammonia, NH3 and 14.00 mL of…

A: Given: Volume of ammonia = 34 mL Molarity of ammonia = 1.0 M volume of water = 14 mL Kb of ammonia =…

Q: Calculate the pH of a solution that has [OH-] = 5.9 x 10 -5 M

A: pH of any solution is given by  pH = 14 + log[OH- ]  where [OH- ] = concentration of OH- ions in the…

Q: Calculate pH and pOH for an aqueous solution containing1.0 × 1 0 -3 mol of HCl dissolved in 5.0 L of…

A: The given data: The moles of the HCl = 1.0×10-3 mol The volume of the solution = 5.0 L To determine…

Q: A solution is made by dissolving 18.4 g HCI (MM=36 g/mol) in 662 mL of water. The pH of the solution…

A: HCl is strong acid

Q: 0.60 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 6.0 L of solution. What is…

A: Molecular weight of NaOH= (23+16+1) = 40 gm/mol  Amount of NaOH taken = 0.6 gm  Moles of NaOH =…

Q: A sample of 7.5 L of NH3 gas at 22 °C and 735 torr is bubbled into a 0.50-L solution of 0.40 M HCl.…

A: The negative logarithmic concentration of hydronium ions in a solution is called the pH of the…

Q: How many moles of NH3 must be dissolved in water to give 813.0 mL of solution with a pH of 11.15? Kb…

A: The value of Kb for the given weak base is = 1.8x10-5 The concentration of the base solution is =?…

Q: Calculate the ph of a solution that is made by dissolving 6.45g of NH4Cl(53.49g/mol) in enough water…

A: First calculate molarity by mole/volume. Then use weak base concept to get pH

Q: If 0.050 moles of gaseous HCl is bubbled in 1.0 liter of a solution that is 0.15 M in NH3 and 0.10 M…

A: When an acid is added to a weak base buffer solution, the concentration of weak base decreases where…

Q: Calculate the pH, pOH, and [OH-1] of solution in which the [H3O+]=1.2x10-3

A:

Q: Calculate [OH-] and pH for each of the following strongbase solutions: (a) 0.182 M KOH, (b) 3.165 g…

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

Q: A solution of formic acid (HCOOH, Ka = 1.8×10-4) has a pH of 2.70. Calculate the initial…

A: The question is based on the concept of chemical equilibrium. we have to calculate initial…

Q: Determine the pH of a solution when 25.7 mL of 0.13 M HNO3 is mixed with 20.5 mL of:   A) 0.100 M…

A: Note: Since you have posted a question with multiple subparts, we will solve the first three…

Q: A solution is made by dissolving 18.4 g HCI (MM=36 g/mol) in 662 mL of water. The pH of the solution…

A: given, mass of HCl = 18.4 g Molar mass of HCl = 36 g/mol Volume = 662 mL

Q: a) Calculate the pH of the solution formed when 100 cm³ of 0.100 mol dm³ H₂SO, is added to 50 cm³ of…

A: Pls repost your question ( 5) .

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the pH of the solution. Calculate the…

A: Applying formula [H+][OH-] = 1×10-14 And PH = -log[H3O+]

Q: The ionization constant for NH3 in water is 1.8 x 10 - 5. Determine the hydrox concentration and the…

A: The dissociation of ammonia in aqueous solution can be represented as: The ionization constant for…

Q: The pH of a 0.23-M solution of HF is 1.92. Determine Ka for HF from these data

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH is given…

Q: Calculate the pH of each solution and indicate whether the solution is acidic or basic.(a) [H3O+] =…

A: pH of the solution is calculated as, pH =-logH+

Q: Calculate the theoretical pH of 10 mM NaOH using the data below: • NaOH is a strong base,…

A: We know that, pH is the negative logarithm of hydrogen ion concentration, i.e.…

Q: Calculate the pH of a solution that is 0.54 M HF and 1.00 M KF. Ka = 7.2x104 pH =

A: Given, Concentration of HF = 0.54 M Concentration of KF = 1.00 M Ka for HF = 7.2 x 10-4  PH = ?

Q: A solution with a volume of 250.0 mL, contains 1.47 g NH, and 3.95 g NH,NO, . a. What is the pH of…

A: The molarity of NH3 and NH4NO3 is: Molarity of NH3 =1.47 g17.03 g/mol×1000250 mL=0.345 MMolarity of…

Q: A chemist dissolves 165. mg of pure sodium hydroxide in enough water to make up 190. mL of solution.…

A: Given,  Weight of pure sodium hydroxide = 165 mg = 0.165 g volume of solution = 190 mL = 0.190 L…

Q: Calculate the pH of solution made by combining 100 ml of 0.28 M HC H,O; and 50 ml of 0.36 M NAOH, Ka…

A: Note: As per our guidelines, we are supposed to answer only one question when multiple questions are…

Q: Determine pH of a solution containing 0.0153 M HClO4 containing 0.105 M NaClO4 .

A: pH = -log[H+]  Given [HClO4]= 0.0153 M

Q: Find the pH of a solution with: [H+] = 1.6×10-6 M pH =

A: Given data, [H+] = 1.6×10-6 M

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH–], of 3.30 x 10-5 M.

A: The acidity or bascity of a solution is defined in terms of pH.pH, mathematically, is -log[H+].…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 9.7×10-2 M. The hydronium ion…

A:

Q: A solution is made by dissolving 27.5 g of HONH3CIO3 in 500.0 mL of water. Using Ka(HONH3*) = 9.1 ×…

A: The amount of HONH3ClO3 dissolved in 500.0 mL of water is 27.5 g. The dissociation constant of…

Q: The pH of a 0.20-M solution of HF is 1.92. Determine Ka for HF from these data.

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: Calculate the pH of 3.0 X 10-5 M Mg(OH)-, which completely dissociates to Mg2+ and OH-.

A: Given that the Mg(OH)2 completely dissociates, so the dissociation reaction is, Mg(OH)2 →Mg2++2OH-

Q: Calculate the pH of the following solutions: a) 0.10M H2SO4  b) (5.0 x 10^-2)M NaOH

A: Sulfuric acid (0.1 M) releases 0.2 M hydrogen ions. The pH can be calculated as: pH = -logH+pH =…

Q: Calculate the pH of a solution that is 0.20 M HOCI and 0.88 M KOci. Kg = 3.5x10-8 pH =

A:

Q: Calculate the pH of a solution prepared from 3.0 g of acetic acid to 500 mL of water.

A: Solution: pH is the measure of hydrogen ion strength of a solution and its value is equal to the…

Q: 0.50 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 4.5 L of solution. What is…

A: In order to calculate pH of the given base sodium hydroxide, follow the below mentioned steps: 1)…

Q: Calculate the ph and poh for a solution that is 0.63 M in NH3 and 0.4 M in NH4Cl, Ki for NH3 is…

A: Given,  The molarity of NH3 = 0.63 M  The molarity of NH4Cl = 0.4 M The Ki for NH3 = 1.9 × 10-5  The…

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: Determine the pH of a 0.068 M aqueous solution of sodium cyanide. The Ka for HCN is 4.9x 10^-10

A:

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.