Answered: (v) Ca(OH)2 is a strong base that…

(v) Ca(OH)2 is a strong base that completely dissociates in solution. What is the pH and pOH of a 0.011 mol L-1 aqueous solution of Ca(OH)2.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 19QAP: . How is the strength of an acid related to the fact that a competition for protons exists in...

See similar textbooks

Related questions

Q: Calculate the pH of Ba(OH)2 solution whose 250 cm3 of a 0.01moldm-3 solution is diluted to 500 cm3…

A: The pH of a solution can be calculated as follows: pH= 14-pOH where pOH = -logOH- To calculate…

Q: The pH of a half-neutralized solution of a weak acid is 4.3. What is the dissociation constant (Ka)…

Q: The pH of black tea is 5.5, while the pH of Coke is 2.5. Which of the following correctly describes…

A: To know the concentration of H+ ion , pH scale is introduced Negative logaritham of H+ ion…

Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…

A: We will calculate the number of moles of each reactant and then draw ICE table to calculate pH of…

Q: The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they…

A: Given: The simplest amino acid is glycine, H2NCH2COOH.

Q: What is the pH of a 0.078 mol dm–3 solution of a diprotic acid which is completely dissociated?…

A: Diprotic acids are those which has two protons to donate. Concentration of diprotic acid[H2A] =…

Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…

A: The dissociation of acetic acid is given as, CH3COOH↔CH3COO- + H+ By definition, the acid…

Q: Acid strength decreases in the series HI > HS04 > HF > HCN. Which of these equal molar salt…

Q: TRIS (also known during medical use as THAM) is an organic compound used extensively in biochemistry…

A: "pH" tends to exhibit the actual potential of H+ ions in specified solution. The solution exhibiting…

Q: The pOH of an aqueous solution of 0.354 M acetylsalicylic acid (aspirin), HC9H7O4, is

Q: What is the pH of a 0.620 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10 4)?

Q: The pOH of an aqueous solution of 0.428 M acetylsalicylic acid (aspirin), HC9H7O4, is

A: Aspirin is a monoprotic weak acid with formula HC9H7O4. Hence it will dissociate partially as per…

Q: 1) Calculate the pH of a solution prepared by dissolving 2.20 g of sodium acetate, CHCOONa, in 78.0…

Q: 1) Calculate the pH of a solution prepared by dissolving 2.35 g of sodium acetate, CH,COONa, in 81.5…

Q: What is the pH of a 0.540 M solution of Ca(NO,), (Ka of HNO, is 4.5 x 10*)?

Q: The pH and Kh of 0.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 :will be respectively…

A: Kh=kWkC pH + pOH = 14 From Ostwald's dilution law , pOH=-logkbxc Where c is the concentration of…

Q: What would be the pH if 1.11 moles of hydrofluoric acid (HF) were added to 2 liters of pure water,…

A: Given : Number of moles = 1.11 pKa = 3.2 HF ⇔…

Q: The acid dissociation constant K, of hydrocyanic acid (HCN) iS 6.2 x 10 10 Calculate the pH of a…

Q: Given a mixture of 100cm3 of 1.01M HCl and 400cm3 of 0.04 NaOH, calculate the pH of the solution.

A: We have given that Volume of HCl = V1 = 100ml Molarity of HCl = M1 = 1.01M Volume of NaOH = V2…

Q: ulate the pH of a solution prepared by dissolving 1.90 g of sodium acetate, CH,COONA, in 85.0 ml of…

A: Given, Mass of Sodium Acetate = 1.90 g Ka of CH3COOH is 1.75×10-5.

Q: The acid ionization constant for a certain monoprotic acid (HA) is 1.57×10−4. What is the pH of a…

Q: In the laboratory, a general chemistry student measured the pH of a 0.591 M aqueous solution of…

Q: The value of K, for phenol (a weak acid) is 1.00×10-10. What is the value of Kp, for its conjugate…

Q: A weak base, BOH, has a ph of 9.80 and Ka equal to 1.0 x 10-5. What is the Molarity of BOH?

A: Given data, The pOH of a weak base is calculated as shown below.

Q: The acid constants of the polyprotic acid НЗASO4 are К_a1 %3D 5х10 ^-3, К_а2 - 8х10^-8, К_а3 %3D…

Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?

A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…

Q: The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the…

A: pH is the negative logarithm of Hydrogen ion concentration. pH of a solution can be calculated as:…

Q: The weak base colloquially known as Tris, and more precisely as tris(hydroxymethyl)-am inomethane,…

A: Buffer solution is the solution which resist to change the pH on the small addition of acid and base…

Q: CH;NH, is a weak base (Kp = 5.0 × 104), so the salt CH,NH,NO, acts as a weak acid. What is the pH of…

A: The pH of salt of strong acid and weak base can be calculated by using formula

Q: The pOH of an aqueous solution of 0.313 M acetylsalicylic acid (aspirin), HC9H704-

Q: Determine the base ionization constant (in x 10^5) of a 0.0925 g sample of week base (molar mass =…

Q: The pOH of an aqueous solution of 0.591 M phenol (a weak acid), C,H5OH, is

Q: If 10 mL of 0.1 M hypothetical acid, HA, is added with 10 mL of 0.1 M of the salt of its conjugate…

A: Answer: The mixture of acid HA and its conjugate base XA will be a buffer solution.

Q: .623 g of NaC2H3O2 are placed in a solution of 0.105 M HC2H3O2 to make 1.00 L of solution. What is…

A: pH is negative logarithm of Hydrogen ion concentration

Q: Given that methylamine, CH3NH2, has a Kb of 4.4 x 10-4, what is the pH of a 0.20 M aqueous solution…

A: For weak base CH3NH2 : [OH-] = Kb×C = 4.4×10-4×0.20 = 9.38 x 10-3 M pOH = - log…

Q: Rainwater is acidic because CO2(g) dissolves in the water, creating carbonic acid, H2CO3. If the…

A: Given: Raindrop pH = 5.60 Sum of [H2CO3], [HCO3-] and [CO32-] = 1.0×10-5 M

Q: The hydroxide ion concentration, [OH*], of an aqueous solution of 0.591 M trimethylamine (a weak…

A: Trimethylamine dissolved in H2O and since it is a weak base so it dissociates partially as follows

Q: A 0.437 M solution of a weak base has a pH of 11.94. What is the base hydrolysis constant, Kp, for…

Q: What is the pH of an aqueous solution of 0.005 M C6H5O- at 298 K of the Ka for phenol at the given T…

A: Given: Concentration of C6H5O- = 0.005 M And Ka of C6H5OH = 1.0 × 10-10

Q: The first acid ionization constant of the oxoacid H;PO, is 8 x 10-2. What molecular structure do you…

A: H3PO2 is a monoprotic acid in aque.

Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10¬1º. Calculate the pH of a…

A: Given, initial concentration of HCN = 3.0 M Ka for HCN = 6.2 x 10-10 The hydrocyanic acid…

Q: The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they…

Q: Write the expressions for the acid dissociation constants for the three successive dissociations of…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 °C. At the same temperature, Ka for HBRO, =…

Q: prepared

A: Equilibrium Reaction is : F^-(aq) + H2O(l) <------> HF(aq) + OH-(aq) Major species are :…

Q: 1) Calculate the pH of a solution prepared by dissolving 1.60 g of sodium acetate, CH3COONa, in 64.0…

A: Given; The given mass of CH3COONa, (W) = 1.6 g. The molar mass of CH3COONa, (M) = 82.0343 g/mol.…

Q: The acid dissociation K, of acetic acid (HCH,Co, is 1.8 x 10 a Calculate the pH of a 2.6 x 10 M…

A: Acetic acid is a weak acid. hence it will dissociate partially as per the reaction CH3COOH ---->…

Q: What is the pH of a 0.680 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 104)?

A: Given, The pKa value of HNO2=4.5×10-4 Molarity of Ca(NO2)2= 0.680M.

Question

(v)
Ca(OH)2 is a strong base that completely dissociates in solution. What is the pH and pOH of a 0.011
mol L-1 aqueous solution of Ca(OH)2.

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

Introduction:

VIEW

Solution:

VIEW

Step by step

Solved in 2 steps

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

Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
At 250°C, the equilibrium constant for the dissociation of water is 10–11.16. At this temperature, what is the pH of a neutral solution?
The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2. What is the pH of a 0.15 molar solution of this acid?
The pH value of the 5L aqueous solution prepared with 6.4 grams of a precious strong acid is 2. So what is the molar mass of the acid?
The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature. What is the initial molar concentration of C5H5N, if its base ionization constant is: Kb = 1.7×10–9?
Discuss the justification for this statement: “Although one does not normally regard NH+4 as an acid, it is actually only slightly weaker as an acid than hydrocyanic acid, HCN, in aqueous solution.”
What is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water tomake 450. mL of solution? Assume that Ba(OH)2 dissociates completely in water to Ba2+ andOH¯ ions. What is the pH of the solution?
Determine the base ionization constant (in x 10^5) of a 0.0925 g sample of week base (molar mass = 17.03 g/mol), B, that is dissolved in water to produce 100 mL of a solution with a pH of 11.00.
The pH of a solution of 0.63 M pyridine is 9.51, what is the Kb of pyridine? What is the Ka of its conjugate acid?
Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COON,, in 53.5 mL of 0.15 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5.
Acidic water can be treated with basic substances to increase the pH, although such a procedure is usually only a temporary cure. Calculate the minimum mass of lime, CaO, needed to adjust the pH of a small lake 1V = 4 * 109 L2 from 5.0 to 6.5. Why might more lime be needed?