Answered: calculate the pOH of [H=] = 2.5 x 10-5…

Science

Chemistry

calculate the pOH of [H=] = 2.5 x 10-5 m a. 9.40 b. 4.0 x10^-10 c. none d. 14.0 e. 4.60

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.82PAE

See similar textbooks

Related questions

Q: What is the pH of a 1.8 x10^-2 M Ba(OH)2 solution? A. 12.56 B. 2.85 C. 4.44 D. 6.38

A: Ba(OH)2 is a strog base. It dissociates completely to gibe Ba2+ and OH- ions Ba(OH)2 --------->…

Q: A 0.010 M aqueous solution of a weak acid HA has a pH of 4.0. What is the degree of ionization of HA…

Q: H+ concentration

Q: What is the pH of 0.2 N perchloric acid (HCIO4, strong acid)? (H=1, 0 =16, CI =35.5)? a. 0.3 b. 2…

A: Given that: Normality of Perchloric acid = 0.2 N pH of Perchloric acid = ?

Q: A. FILL IN THE TABLE. Calculate pH from the following hydrogen ion concentration (M). Identify each…

A: (A) pH is Negative logarithm of Hydrogen ion concentration. If it's value equal to 7 then Substance…

Q: Acid pH of 0.10 mol/L solution HNO (AQ) 1.0 HNO₂(AQ) 2.2 1. Nitric acid and nitrous acid are two…

A: Acidity is defined as the ability of a molecule to release protons. if a compound easily donate…

Q: Find the pH of the following acidic solutions: A 0.001 M solution of HCl (hydrochloric acid). 3…

A: 'As you have posted multipart question, we will solve first three. If you want any specific part to…

Q: 13a. What is the pH of a solution with [OH−] = 5.5x 10-9M? A. 5.7 B. 0.7 C 9.7 D. None of…

A: pH of a solution is given by the negative logarithm of the hydrogen ion concentration of the…

Q: What is the concentration of H+ in a pH 0 solution of acid? A. 0 M B. 1 M C. 1 X 10-7 M D. 1 X…

A: 1 M -------> option(B)

Q: A solution which contains 0.10 M KOH has a pH which is ___________ that the pH of a solution which…

A: pH = -log H+pOH = -loh OHpH +pOH = 14Given , KOH = 0.10 mCA(OH)2 = 0.10 mpH = ?

Q: -117. Determine [OH¯], [H*], and the pH of each of the following solutions. a. 1.0 MKCI b. 1.0 M…

A: Given,1.0 M KCl1.0 M KC2O2

Q: solution with a pOH of 10.70 has an [H +] of a. 2.0 × 10−12 M. b. 5.0 × 10−4 M. c. 3.2 × 10−4 M.…

Concept explainers

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.

Question

calculate the pOH of [H=] = 2.5 x 10-5 m

a. 9.40

b. 4.0 x10^-10

c. none

d. 14.0

e. 4.60

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The pOH of 0.23 M C6H5NH3* (Ka = 2.51 x 105) at 25°C is: (Given that: C6H5NH3* + H2O → C6H5NH2 + H3O*) O a. 9.35 O b. 2.60 О с. 8.53 O d. 11.4 е. 10.5
Final Volume V₂ = 341 mL al Volume V₁ =? 10. What is the molecular geometry and molecular polarity for CH₂Cl, and SO, ²? 11. What do catalysts do and how do they affect reaction rates? 12. 2 Atoms are side by side. Their chemical reactivity is dependent on the electrons which hold serve fe 13. Identify the acid, base, conj. Acid, conj. Base: H₂CO, + HPO4 H₂PO4 + HCO, 14. True or False? Chemistry looks at the microscopic view of matter. 15. Identify the 4 biological buffer mechanisms 16. Calculate the density of silver metal if 930 cm³ block has a mass of 2.21 x 104 g. Express the answer with the correct number of significant figures. 17. Kinetic molecular theory describes the behavior of which state of matter? 18. The pH scale operates on a logarithm scale which means an increase or decrease fold in the of pH is by 10s. So, a change in pH from 5 to 3 is a hydrogen ion concentration. And in other words, a pH of 3 has and less OH- than a pH of 5 19. A precipitate occurs in the reaction…
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H+] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.735, the hydrogen ion concentration is mol/L.
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H¹] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.171, the hydrogen ion concentration is mol/L.
At 25.0 oC, Kw = 1.0 x 10-14 and neutral water has a pH of 7.00. At 98.4 oC, Kw = 5.11 x 10-13 and neutral water has a pH of _____. Record your answer to 3 decimal places.
Pls do Asap...! Pls do que 1 as soon as possible
The value for Kw is 1.0 X 10-14 in all aqueous solutions, regardless of pH. Thus, the value for Kw in vinegar (5 M aqueous acetic acid) is __________. 1.0 X 10-14 2.5 X 10-3 5.0 X 10-14 1.0 X 10-7
1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.
12. Select the TWO expressions that represent the following system: Et „N (aq) + PHNH,+(aq) PHNH, (aq) + Et NH+ (aq) K, Et „NH+ x K. PHNH,+ a K O K, b PHNH, K. Et N K Et NH+ x K · PHNH,+ x K a a 3 Et„N x K K, , Et ¸N PHNH, + х к K, PHNH , O K, Et t;N × K, p, PHNH, b 2 K O K, , Et N x K, PHNH,+ a K O K, , E ¸N × K, · PHNH, х к 9. K K, , Et ‚N × K,, PHNH, K, Et „N x K b. 3 2 K, , PHNH,
Can you please show me the computation or how to compute? Thank you.
The concentration of hydronium ion in a sample of a solution is 4.5 x 10-3 mol/L. What is the pH of this solution? The answer should be to the proper number of significant digits
CHEMISTRY RATE WILL BE GIVEN! NO LONG EXPLANATION NEEDED. PLEASE ANSWER 47-52