Answered: If [OH" ] = 5.2 x 10-4 M, what is the…

Science

Chemistry

If [OH" ] = 5.2 x 10-4 M, what is the pH ? pH РОН [H* ] [OH ] ? 5.2 x 10-4 M O -3.3 O 10.7 O -10.7 O 1.9 О 3.3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: If pH of a solution of NaOH is 12.3, then what is the value of [H+] ? O 12.3 M O 5.01x10-13 M O 5.01…

A: Given that the pH of a solution of NaOH is 12.3. To calculate the [H+] of the given solution.

Q: Determine the [OH-], pH, and pOH of a solution with a [H*] of 3.5 x 10-1" M at 25 °C. [OH¯] = M pH :…

A: For part 1: given [H+] =3.5 x 10-11Mwe know that, [H+][OH-] =10-14…

Q: Calculate the [OH] and the pH of a solution with an [H] = 5.6 x 10-¹0 M at 25 °C. [OH-] = pH =…

Q: Calculate the (OH| and the pH of a solution with an [H*] = 6.7 x 10-8 M at 25 °C. %3D 3D[_HO] pH =…

Q: Calculate [OH-] and pH for a 1.5 x 10-3 M solution of Sr(OH)₂. b. a. [OH-] = 3 × 10-³ M; pH = 16.52…

A: The objective of this question is to calculate the concentration of hydroxide ions [OH-] and the pH…

Q: Determine the [H+], [OH-], and pOH of a solution with a pH of 3.20 at 25 °C. [H+] = [OH-] = pOH =…

A: Part 1 pH = 3.20 [H+] = ? [OH-] = ? pOH = ?

Q: Notion of PH Examples: 1- Calculate the PH of the following solutions: Solution A: [H30+] = 10-2…

A: 1) We know, PH= - log [H3O+] [H3O+]=Concentration of H3O+ Solution A: PH= - log(10-2) Or, PH=2…

Q: A solution of H2SO4 has a concentration of 4.2 × 10-8 M. Its pH is 7.00. O True O False

A: PH = - log(H+) H2SO4 has basicity 2, means it release 2 proton (H+) So, concentration of H+ = 2*…

Q: find the pH and [OH-] if [H3O] = 7.8 x 10^-8

Q: Which of the following relationships in incorrect? Assume 25°C. a. pH + pOH = 14.00 b.…

A: b. [OH-] = 10pOHExplanation:Incorrect Option:Option b:[OH-] = 10pOH: This relationship is…

Q: [H;O*] [OH] pH 0.40 РОН Acidic or Basic? 9.01 x 10-10 1.0 x 108 2.00 4.5 x 102

A: We can use the equation [H+][OH-] = 10-14 is equal to ionic product of water,It is used to…

Q: 2. Calculate the following (report to 2 decimals, use scientific notation when calculating H3O*) and…

A: In a given question we have to find out pH of a solution i.e. pH= -log[H3O+] If pH>7 Basic…

Q: Which solution has the highest pH? O 0.065 M HIO (Ka-2.3x10-11) O 3.5x10-4M HBrO (Ka-2.5x10-9) O…

Q: For the diprotic weak acid H₂A, Kal = 3.2 × 106 and K₁2 = 7.6 × 10⁹. What is the pH of a 0.0800 M…

Q: Which one is correct? What is the [H3O+] in a solution with pH=8? 10+8 M 10-8 M 8.0 M 6x10-8 M…

A: Given, pH = 8 PH is defined as negative logarithm of concentration of [H+] ion.

Q: 8. What is the pH of a cup of coffee that has a [OH-] of 1.200 x 10-10?

A: Detail mathematical calculation is shown below

Q: Determine the H+], pH, and pOH of a solution with an OH-] of 3.3 x 10-12 M at 25 °C. [H*] M…

Q: alculate the pH of the following solutions. a) [H3O*] = 1.0×10-4 M pH=| b) [H;O*] = 0.10 M pH = «)…

Q: What is the pH of neutral water at 40 °C? [H3O+] = [OH-] = 1.71 x 10-7 M pH = -log[H3O+] pH = [?]

Q: 12) The pH of a solution is measured to be 10.40. What are the values of [H3O+] and [OH-] for this…

A: The pH of the solution = 10.40 H3O+=?OH-=?

Q: Which of the following relationships in INCORRECT? Assume T = 25°C. a pH + pOH = 14.00 b…

A: Temperature = 25◦c = (25+273) = 298 K pH = -log[H+] = -log[H3O+] pOH = -log[OH-]

Q: [H;O1+] 9.84 x 109M

Q: The [H3O+] of lemon juice is 2.5 x 10-2 M. Calculate the pH.

A: Given [ H3O+ ] = 2.5 × 10-2 M PH = ?

Q: what is the pH for [OH−]M_1 = 2.9×10−7 M [H3O+]M_2 = 4.4×10−3 MM [H3O+]M_3 = 2×10−4 M

A: Given :- [OH-] = 2.9×10−7 M [H3O+]= 4.4×10−3 M [H3O+]= 2×10−4 M To calculate : pH in each part

Q: Which of the following solutions is acidic? O [H3O+] = 1.0 x 10-7 M O [H3O¹] = 1.5 x 10-1⁰ M O…

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H, O0*], of 5.24 × 10-³ M.

A: pH is defined as the negative logarithm of the activity of hydronium ion. But in dilute solutions,…

Q: For the diprotic weak acid H2A, Kal = 3.5 x 10-6 and Ka2 = 7.7 x 10-9. What is the pH of a 0.0400 M…

A: Ka1>> Ka2 it means second dissociation is very small

Q: Determine the H*|, pH, and pOH of a solution with an OH-] of 4.2 x 10-12 M at 25 °C. [H*] = M %3D pH…

Q: What is the [H*] of an acid solution that has a pH of 3? 1 x 10-3 M 0 1х1011 М 1 x 1011 M О 1х103 М

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

Q: Determine the [H*], [OH-], and pOH of a solution with a pH of 1.90 at 25 °C. [H*] : M [OH"] = M pOH…

A: Given, PH = 1.90 PH us defined as negative logarithm of concentration of H+ ion.

Q: Given an OH concentration of 0.10 M, calculate the H30* concentration, then identify the solution as…

A: [OH-] = 0.10 M Since we know that, [H3O+] × [OH-] = 1.0 × 10-14 [H3O+] = 1.0 × 10-14 / 0.1 = 1.0 ×…

Q: A solution has a pH of 3.4, what is [H*]? 2.51 x 10-11 M 3.4 M 3.98 x 10-4 M 07M

A: pH of a solution is defined as the negative logarithm of hydronium ion concentration.…

Q: Calculate the [OH-] and the pH of a solution with [H] = 3.0 x 10 Mat 25 °C. [OH-] = [H*] = Calculate…

A: The objective of the question is to calculate the concentration of hydroxide ions and the pH of a…

Q: HCI has a pH of 3. What is the concentration [OH-]?

Q: The [H3O+] of ammonia is 8.3 x 10-11M. What is the pH of ammonia? Use 2 decimal places for pH.

A: Given, [H3O+] of ammonia is 8.3 × 10-11 M [H3O+] = 8.3 × 10-11 M pH of ammonia = ?

Q: Calculate the [H*] in a solution that has a pH of 9.16.

A: Given :- pH of solution = 9.16 To calculate :- [H+] i.e. hydrogen ion concentration

Q: pH=-log[H+] [H+]=10-pH pH+pOH=14 pOH=-log[OH-} what is the pH of 0.2 M of Ca(OH)2

A: From ionic product og water, [H+] x [OH-] =10-14…

Q: What is [H+] concentration if pH=0?

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 bleach solution that has a [OH-] = 6.0 x 10-6 M? pH Incorrect Is bleach acidic,…

A: The pH of the solution shows that the solution is acidic, neutral or basic. If the pH is less than…

Q: Which of the following is the most acidic (lowest PH) pOH of 2.0 [OH-] = 1 x 10-7 m [H+]=4.6 x…

A: Given solutions: pOH of 2.0 [OH-] = 1 x 10-7 M [H+]=4.6 x 10-6 M [OH-] = 1 x10 -8 M pH of 9.5 We…

Q: 9.) Calculate the pH, pOH, [0H ], and [H30*] for each solution and determine if acidic or basic.…

Q: The Ka for lcarbonic acid is 1.8 × 10–5. Which of the following statements best describes the pH of…

A: The objective of this question is to determine the pH of a 0.0010 M solution of carbonic acid, given…

Q: If pH = 9.3, what is [H* ] ? pH pOH [H*] [OH ] 9.3 ? O 2.0 x 10° M O 1.1 x 10-15 M O 2.0 x 10-5 M O…

A: The pH of any solution can be determined by using the following formula : pH = - log [H+]

Q: Calculate the pH for the following concentration: [H,0*] = 2.19 x 10-5 M A. pH=4.7 B. PH=4.9 C.…

Q: Carbonic acid, H2CO3, is a diprotic acid. Calculate the concentration of all species (H2CO3, HCO3-…

Q: calculate pH of A) 5.0 x 10-5 M H+ B) 3.4 x 10-11 M H+ C) 2.1 x 10 -4 M H+ D) 1.3 x 10-3 M H+

Question

100%

If [OH ] = 5.2 x 10-4 M, what is the
pH ?
pH
РОН
[H* ]
[OH ]
5.2 x 10-4 M
O -3.3
O 10.7
O-10.7
Ο 1.9
О 3.3

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Determine [OH–], pOH and pH of a 0.63 M aqueous solution of LiC3H5O3 (K b = 7.1×10-11).
[H3O+1] = 10-PH [OH-1] = 10-pOH [H3O+1][OH1] = 10-14 pH - log [H3O+1] = %3D pOH = - log [OH-] pH + pOH = 14 %3D %3D What will be the pH if 0.00150 moles of HCl is added to 1.00L of water ? The reaction gives the conversion factor HCI + H2O H3O+1 + CI1 start: 0.00150 equil: O A. 1.5000 В. 2.5223 C. 2.824 D. 3.125 Е. 6.502
A Determine the [H+], pH, and pOH of a solution with an [OH-] of 0.00011 M at 25 °C. [H*] = pH = pOH = Determine the [H+], [OH-], and pOH of a solution with a pH of 3.79 at 25 °C. [H+] = [OH-] = pOH = Determine the [H]. [OH-], and pH of a solution with a pOH of 4.43 at 25 °C. [H+] = [OH-] = pH = M M M M M
Calculate the pH. [НЗО"1[он], Ка аля а yalues 1.0 М pH [H30*] [OH] pH HC2H3O2 [H3O*] [OH] pH [H3O*] [OH] 0.02 HCI 2.30 11.8 NH3(ag) H2O = H;Ơ + CĨ HC1 HC2H3O2 H20 H;Ơ + C,H;O [C,H;O2] [H;Ơ] NH3 + H2O OH NH4 [NH) = [OH]
The Ka for lcarbonic acid is 1.8 × 10–5. Which of the following statements best describes the pH of a 0.0010 M solution of carbonic acid? The pH is exactly 7. The pH is exactly 3. The pH is greater than 7 but less than 12. The pH is greater than 0 but less than 3. The pH is greater than 3 but less than 7.
What is the pH of 3.0 × 10-³ M HCl? pH = What is the pH of 8 × 10-8 M HCl? pH =
What is the pH of a 0.0235 M H* solution? Formulas [H*] = 10-PH [OH-] = 10-POH H* OH [H]-1x 104 TOH] pH = - log,o[H*] pOH = - log.,[OH-] OH - 14- pH pH + pОН %3D 14 pH РОН pH-14 pOlH -1.63 O 1.63 O 42.66 O 12.37 01-110
True or False. Write TRUE if the statement is correct and FALSE if it is incorrect. ___________1. Given HA yields H+ + A-, its =[HA]/[H+][A-] ___________2. In determining pH, the [H-] is used. ___________3. Given pOH = -log [OH-], [OH-] = 10pOH.
A diprotic acid (H, A) has Ka1 = 4.27 x 10-7 and Ka2 = 5.98 × 10-11. What is the pH of a 0.437 M H, A solution? pH =
Determine the [H*], [OH], and pOH of a solution with a pH of 5.95 at 25 °C. [H*] = 1.122 x10 M [OH] = 8.9 x10-9 M РОН 3 5.95 Determine the [H*], [OH¯], and pH of a solution with a pOH of 2.14 at 25 °C. [H*] = M Incorrect [OH"] = M Incorrect pH Incorrect
What is the pH of a 0.063 M solution of hypoiodous acid (HIO)? Ka for HIO is 2.3x10-¹¹.
Determine the pH of 1.5 M HBrO. (Ka HBrO = 2.5 x 10–9)