Find [OH−] and pH for a 0.022 M solution of Sr(OH)2

Q: (b) What are [H3O+], [OH -], and pH in a solution with a pOH of 4.19?

A: Since we know that pH + pOH = 14  => pH for the above case = 14 - pOH = 14 - 4.19 = 9.81

Q: is the salt Sr(NO2)2 acidic, basic, or neutral?

A: When a weak acid and a strong base are mixed, they react according to the following net-ionic…

Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: The pH of a solution that contains 0.010 M H3O+ is

A: The concentration of [H3O+] = [H+] = 0.01 M.

Q: What is the pH of a 0.116 M solution of KOH?, and a 0.116 M solution of Ca(OH)2 ?

A: Step 1: Step 2:

Q: A) In the lab, you're working with a solution and measure it's pH with a meter to be 6.9. However,…

A: We know that, pH is the negative logarithm of hydronium ion concentration and pOH is the negative…

Q: 1. Calculate the following for the given aqueous solutions at 25.0 oC:​a) The pH of a 5.75 x 10–8 M…

A: The solution is given below -

Q: What is the pH of a 0.020M Sr(OH)2 solution?

A:

Q: What is the pH of a 0.370 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: Given : Concentration of Ca(NO2)2 = 0.370 M And Ka of HNO2 = 4.5 X 10-4  Since Ca(NO2)2 is a…

Q: Calculate the pH of a 0.043 M NaF solution. (K, for HF = 7.1 x 104.)

A: Given -> Molarity of NaF = 0.043 M Ka ( HF) = 7.1 × 10^ -4

Q: 12. Calculate [OH] for a solution of pH = 5.88.

A: An acid base reaction is also called as neutralization reaction. The H+ ions of acid react with OH-…

Q: At 25°C, calculate the pH of a 0.426 M solution of the salt KNO2. (Ka (HNO2) = 4.50 × 10−4 ).

A:

Q: Calculate the pH of a 0.020M solution of Sr(OH)2 Calculate the pOH of a 0.020M solution of Sr(OH)2.

A:

Q: A sample of Ca(OH)2 with a mass of 0.151 g is dissolved in water so that the volume of the solution…

A:

Q: Calculate the pH of a 1.60 M KBrO solution. Ka for hypobromous acid, HBrO, is 2.0 × 10

A: In case of conjugate acid-base pairs,  Ka is acid dissociation constant and Kb is base dissociation…

Q: Example2: Calculate [H;0"], [OH] concentration and pH and pOH of 0.2 M aqueous solution of NaOH.

A:

Q: Calculate the pH of the following solution 7.1 × 10−4 M Ba(OH)2:

A: Concentration of Ba(OH)2  is 7.1×10-4 M 1 mol Ba(OH)2  = 2 mol OH-,  So concentration of OH- is =…

Q: Give two different pH values, explain the relative differences in concentration of H+ between the…

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What is the pH of a 0.0250 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: pH can be calculated as follows

Q: What is the pH of a solution that is 0.080 M in NaClO at 25 °C?  The Ka for HClO is 4.0×10^-8

A: NaClO is salt made by strong base sodium hydroxide and weak acid HClO

Q: What is the pH of a 0.320 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A:

Q: What is the pH of a 0.720 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: Determine Ka for hydrogen sulfate ion, HSO4 −. In a 0.10-M solution the acid is 29% ionized.

A:

Q: What is the [OH-] of this solution?

A: pH + pOH = 14  pH = -log [H+]  pOH = -log [OH-]   [H+] = 10-pH  [OH-] = 10-pOH

Q: Calculate the pH of a 0.022 M RbOH solution.

A:

Q: What is the pH of a 0.0000100 M solution of CsOH?

A: Given :-  Concentration of CsOH = 0.0000100 M   To calculate :-  pH of solution

Q: The pH of a 0.0040 M solution of Ca(OH)₂ is

A: Given, Concentration of Ca(OH)2 solution = 0.0040 M So, [OH-]= 2×0.0040 M= 0.0080 M

Q: The pH of the 0.50 M solution of HA is 1.92. What is [HA]?

A: Answer:pH is equal to negative of logarithm of hydrogen ion concentration in solution, so,

Q: What is the pH of a 0.820 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The pH of the solution is equal to the negative logarithm of hydronium ion while pOH of the solution…

Q: Calculate the pH of a 0.600M solution of zinc nitrate, Zn(NO₃)₂

A: Given, Concentration of zinc nitrate, Zn(NO₃)₂ = 0.600 M

Q: 10) What is the pH of an Al(OH)3 solution with a concentration of 0.0182 M?

A:

Q: What is the pH of a 0.830 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The chemical equation may be written as: The given data is: Concentration of Ca(NO2)2 =0.830M Ka of…

Q: The pH of an acidic solution is 3.37. What is [H⁺]?

A:

Q: What is the pH of a solution that is 0.080 M in NaClO at 25 °C? The Ka for HClO is 4.0*10^-8

A:

Q: 6. Calculate the pH of the solution if the concentration of [H3O] ion is 2.0x10 M at 25°C.

A:

Q: Calculate [OH−] for a solution where [H3O+]=0.00311M.

A: Given data, Concentration of H3O+, [H3O+] = 0.00311 M  We have to calculate concentration of OH- of…

Q: Observations: Note the pH of each solution you test. Record if the solution is acidic, basic, or…

A:

Q: What is the pH of a 0.0610 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A:

Q: (a) blood, pH = 7.50 acidic Obasic neutral (b) gastric juice, pH = 2.50 acidic Obasic M neutral M

A:

Q: What is the pH of 0.350 M Sr(OH)2 ?

A: pOH of the solution is equal to the negative logarithm of hydroxide ion while the pH of the solution…

Q: Question 3 A student is given a concentrated solution that is supposed to contain vinegar, a weak…

A: A weak acid will not be completely dissociated in a solution. However, a strong acid will be…

Q: Calculate 3OH-4 and pH for 2.250 g of LiOH in 250.0 mL of solution,

A: Molarity (M) It is the number of moles of solute dissolved in volume of solution in liters. M=number…

Q: pH = 6.35

A: