of the K, of a monoprotic weak acid is 2.7 x 106, what is the pH of a 0.48 M solution of this acid?DIALO- на14$1014111815%5a306&L18➡+861K◄◄6.D11011|4CO9962°F(12++[inser}

Answered: Image /qna-images/answer/98cd2505-b8a7-46ff-a466-ce2e77e4f83c.jpg

Answered: f the K, of a monoprotic weak acid is…

Science

Chemistry

f the K, of a monoprotic weak acid is 2.7 x 10-6, what is the pH of a 0.48 M solution of this acid? pH =

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 the K₂ of a monoprotic weak acid is 5.9 x 106, what is the pH of a 0.22 M solution of this acid?

Q: The K, of propanoic acid (C,H,COOH) is 1.34 × 10-³. Calculate the pH of the solution and the…

Q: Hydrocyanic acid, HCN, is a weak acid (Ka = 4.02*10-10). If I dissolve 0.882 g of HCN in enough…

A: Given information is as follows: The amount of HCN = 0.882 g The volume of water = 600 mL The value…

Q: The pH of a chemical solution is given by theformula pH = - log10 [H+ ] where [H+ ] is the…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Four solutions of an acid dissolved in water are sketched below, as if under a microscope so…

A: According to Arrhenius concept, an acid is a substance i.e. when dissolved in water gives H+ ions .…

Q: An aqueous solution containing only hydroiodic acid has a [HI] of 0.008002 M. What is the pH of the…

Q: In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…

Q: The pH of 0.259 M solution of an unknown acid is measured to be 2.353. What is the Ka of the acid?

Q: Can you please answer sub question A and B and show all of the steps to the solution please and…

A: In the above problem the solutions are buffer solutions So we will use Henderson Hasselbalch…

Q: 2. Calculate pH and pOH for each of the following solutions and determine whether the solution is…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31. What is the Ka of the acid?

A: Given pH = 2.31 Concentration of acid = 1.86 M Ka =?

Q: The pH of an aqueous solution of 0.534 M methylamine (a weak base with the formula CH3NH2) is

Q: 17) A weak base, B, has a concentration of 0.155 M. If the pH of the solution is 11.24, what is the…

Q: Consider the following ions: Cl-, HS-, NO2-, F-, and HS04-. (a) Which of these ions in water gives…

A: Given ions Cl- HS- NO2- F- HSO4-

Q: The pH of dissolving 1.48 g of propanoic acid (CH3CH2COOH, Ka 1.3X105) in 200 mL H20 is 4.82 O 3.71…

Q: If 31.4 mL of a 0.75 M NaOH solution is added to a 47.1 mL sample of a 0.75 M weak acid, HA, what is…

A: Molarity of NaOH, M=0.75 M Volume of NaOH, V=31.4 mL Millimoles of NaOH=M x V (in mL)= 0.75 x 31.4…

Q: What is the pH of an aqueous solution of 0.159 M sodium cyanide (NaCN)? (Kb of CN- = 2.5 x 10-5)

A: Given, The concentration of sodium cyanide (NaCN) = 0.159 M Kb for CN- = 2.5 x 10-5. pH is the…

Q: A 20.6 mL sample of 0.382 M diethylamine, (C₂H5)2NH, is titrated with 0.272 M hydroiodic acid. At…

Q: What is the pH of a 0.1250 M CH3NH3Br? Kb for CH3NH2 is 3.70e-4.

A: Given, The pH of a 0.1250 M CH3NH3Br is : Kb for CH3NH2 is 3.70e-4.

Q: The following questions refer to a sodium hypochlorite (NaCIO) solution. HCIO K₂ =2.9 x 10-8 a)…

A: NaClO is a salt of weak acid and strong base. pH of this solution can be calculated by the following…

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

Q: A certain solution was found to have a pH of 5.50. Which of following statements is true about this…

Q: The lactate ion, C,H,O7 (aq), reacts with water to form lactic acid and hydroxide ion. C,H;05 (aq) +…

A: Given : [OH-] = 5.2 x 10-6 M So as per ICE table x = 5.2 x 10-6 M

Q: If a buffer solution is 0.170 M in a weak base (?b=3.7×10−5) and 0.540 M in its conjugate acid, what…

A: In question it is not mentioned whether the base is monoprotic or polyprotic. Hence assuming it to…

Q: For the diprotic weak acid H,A, Kal = 3.2 x 10 and Ka2 = 6.3 x 10-9 What is the pH of a 0.0800 M…

A: For H2AKa1 = Ka2 = Concentration of H2A = 0.0800 MWe have to determine the pH of the solution and…

Q: A generic base, B¯, is added to 30.00 L of water. The pH of the solution is found to be 9.05. What…

A: The hydrogen ion [H+] concentration in the solution having a pH of 9.05 is calculated as shown…

Q: If 34.6 mL of a 0.68 M NaOH solution is added to a 51.9 mL sample of a 0.68 M weak acid, HA , what…

A: 34.6 mL of a 0.68 M NaOH solution is added to 51.9 mL sample of a 0.68 M weak acid, HA (ka = 1.8 x…

Q: It is believed that a bath in Epsom Salts can relieve various types of pain. In preparation for…

Q: Pyridine, C5H5N, is a bad-smelling liquid, that is also an excellent solvent. It is used to…

A: The question is based on the concept of pH of the solution. it is defined as a negative logarithm…

Q: Morpholine is a common additive used for pH adjustment in fossil fuel and nuclear power plant steam…

Q: HCl(aq) + H₂O(l) ⇒Cl¯(aq)+ H3O+ (aq) does water act as a Brønsted-Lowry acid, a Brønsted-Lowry base,…

A: we have to determine of water acts as Bronsted Lowry acid or base in the given reaction

Q: Please answer these questions on your Page 8 HA(aq) is a weak acid with a dissociation constant, K₁,…

Q: what is the pH?

A: Given :- Concentration of weak base = 0.120 M Concentration of conjugate acid = 0.590 M Kb = 5.9…

Q: Please answer these questions on your Page 8 (a) 1 ) HA(aq) is a weak acid with a dissociation…

Q: Hypochlorous acid, HOCl, is a weak acid having a pKa = 7.46. (a) Show the balanced chemical equation…

A: Given that : For HOCl, pKa = 7.46 We need to find pKb and pH of solution when [OCl-] = 0.050 M

Q: For the diprotic weak acid H2A, Kal = 3.7 x 10 ° and Ka2 = 6.9 x 10–9 What is the pH of a 0.0600 M…

A: Ka1 and Ka2 values of a diprotic weak acid are given as 3.7×10-6 and 6.9×10-9 respectively.

Q: If the molar concentration of OH- is 1.0 x 10-7, the pH is what?

A: Applying formula of pH POH= -log[OH-]

Q: The pH of an aqueous solution of 0.506 M methylamine (a weak base with the formula CH3NH₂) is

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

100%

of the K, of a monoprotic weak acid is 2.7 x 106, what is the pH of a 0.48 M solution of this acid?
DIALO
- на
14
$
101
4
1118
15
%
5
a
30
6
&
L
18
➡+
8
61
K◄◄
6.
D
110
11|4
C
O
99
62°F
(12
+
+
[
inser
}

Expert Solution

Step 1

Step by step

Solved in 2 steps with 2 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

What is the approximate K for the following acid/base reaction? H25 (aq) +F (aq) ++ HF (aq) +HS (aq) ACID BASE HCI C H2SO4 HNO3 H30 (aq) HSO H3PO4 HSO NO3 H2O so, H,PO, F HF CH3COOH H,CO3 H,S H,PO, NH, CH;COO HCO, HS HPO, NH, CO PO OH HCO HPO. 1,0 OH H, CH CH, OA unable to determine OB. K.<1 Base strength increasing Acid strength increasing
A lake has a surface area of 18 square kilometers and an average depth of 6 m.The average pH of the lake is 6.9. How many tons of acid rain—in the form ofH2SO3—would reduce the pH of the lake from 6.9 to 3.2?
C9a-7
The pH of an aqueous solution of 0.508 M phenol (a weak acid) , C6H5OH, is _______.
The K, of a weak monoprotic acid is 1.65 x 10-5. What is the pH of a 0.0859 M solution of this acid? pH =
The base protonation constant K, of allantoin (C,H¸N,O,NH,) is 9.12 x 10 °. 4 3 Calculate the pH of a 0.46 M solution of allantoin at 25 °C. Round your answer to 1 decimal place. pH = || %D
What mass of aluminum hydroxide can be dissolved in a solution whose pH is held at 11.20? (Ksp of aluminum hydroxide = 1.9x10^-33)
20.
CH, NH, is a weak base (K, = 5.0 x 1o4), so the salt CH,NH,NO, acts as a weak acid. What is the pH of a solution that is 0.0590 M in CH,NH,NO, at 25 °C? pH =
Problems 285 23. The NMR spectra are shown in parts a, b, c, and d for four isomeric compounds with formula CH1202. Their infrared spectra show strong bands near 1735 cm', Make no attempt to inter- pret the aromatic proton area between 7.0 and 7.5 ppm except to determine the number of pro- tons attached to the aromatic ring. Draw the structures of the compounds. C10H1202 4.84 7.0 2.06 2.05 3.01 (a) C10H1202 in 3M 4.94 7.0 2.08 2.04 3.13 3.0 (b)
A.) What is the pH of a 6.18×10-2 M aqueous solution of potassium nitrite, KNO2?pH = This solution is acidic basic neutral? B.) What is the pH of a 0.264 M aqueous solution of ammonium bromide, NH4Br ?pH = This solution is acidic basic or neutral? . .
a) Write the formula for the conjugate base of HPO,2 b) Write the formula for the conjugate acid of NH;