-3 The pH value of a (0.062 + 0.002) mol dm HCI solution is: Select one: 1.21 0.11 1.21 1 1.21 0.01 1.91 + 0.01

Q: (a) Calculate the percent ionization of 0.125 M lactic acid (Ka= 1.4 × 104). (b) Calculate the…

A: a.

Q: enzoic acid (HBenz) has a Kvalue of 6.3 × 10-5. You need to prepare a buffer having a pH a of 4.05…

A:

Q: An aqueous solution contains 0.132 mol L-1 of HCl and 0.717 mol L-1 of acetylsalicylic acid (Ka =…

A: Acetylsalicylic acid is a weak acid and HCl is a strong acid.…

Q: If the Kp of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH 0.00511…

A: Given : Initial concentration of weak base B = 0.47 M Kb of base = 2.4 X 10-6  Since B is a weak…

Q: Calculate the pOH of a 0.75 M weak acid solution at 25°C given a Ka = 1.7 x 10-8

A: Given :- concentration of weak acid = 0.75 M  Ka of acid = 1.7 × 10-8  To be calculated :-  pOH of…

Q: b) Prepare 1000 of pH 5.50 acetate buffer solution from 0.1000 M CH;COOH and 0.1000 M NaCH;CO0…

A:

Q: MISSED THIS? Read Section 18.4 (Pages 803-817); Watch KCV 18.4B, IWE 18.7 Part F Calculate the pH at…

A: Introduction: An acid is defined as a substance that can donate protons and a base that can accept…

Q: Determine the pH of a 0.50 M NaF solution. The Ka of HF is 3.5 x 10-5. Enter the result to 2 decimal…

A:

Q: Calculate the pH at 25 °C of a 0.46M solution of sodium propionate (NaC,H,CO,). Note that propionic…

A:

Q: The Ka for benzoic acid is 6.5  10-5. Calculate the pH of a 0.10 M benzoic acid solution.

A: Benzoic acid is a weak acid so it will not completely be dissociated in its aqueous solution.…

Q: Calculate the pH after addition of 22.55 mL of 0.1298 M HBr to 25.00 mL of 0.1529 M CH 3NH 2. K b(CH…

A:

Q: The base dissociation constant for 2,5-pyridinediamine is Kb=3.0×10−8. Determine the pH of a 0.015…

A:

Q: H2C2O4 = HC2O4- + H+              Ka = 0.0540 HC2O4- + H+ = H2C2O4            K = ? Solve for the…

A: Solve for the equilibrium constant when the dissociation of oxalic acid is reversed.

Q: It is desired to buffer a solution at pH = 4.30. What molar ratio of CH3COOH to NaCH3CO0 should be…

A:

Q: Water sample has a pH of 10. Compute the total alkalinity if the concentration of [HCO3], [CO32] and…

A: Given :          [HCO3-] = 61 mg/L CaCO3           [CO32-] = 167 mg/L CaCO3             [OH-] = 5…

Q: PH value 9.45 using 0.3 M Na2CO3 and 0.2 M HCl How much of each solution to prepare the 1 L buffer…

A: Solution:

Q: What is the pH of a buffer solution containing 1.25 M NH3 and 0.78 M NH,NO3? The base dissociation…

A: NH3 is a weak base and NH4NO3 is its salt , so they form a basic buffer solution. We first use…

Q: A) 0.20 M lactic acid B) 0.20 M lactate C) 0.10 M lactic acid and 0.10 M lactate D) 0.15 M lactic…

A: When there is a buffer solution of weak acid and its salt with equal concentrations of acid and…

Q: 40. 0.05 mol of ammonium nitrate, NH-NCs was dissolve in water in a mL volumetric flask. Compute the…

A: Number of moles of ammonium nitrate, NH4NO3 = 0.05 mol Volume of the flask = 100 mL = 0.100 L (1 L =…

Q: Calculate the pH of a solution formed by mixing 15.0 mL of 0.250 M HClO with 15.0 mL of 0.315 M…

A:

Q: Calculate the concentration of malonate ion (C3H2O42–) in a 0.200 M solution of malonic acid…

A: Given, Concentration of malonic acid, C3H4O4 = 0.200 M For malonic acid, Ka1 = 1.4 × 10–3 Ka2 = 2.0…

Q: Calculate the pOH of a solution containing 0.35 M sodium acetate (NaCH3CO2). The Ka for acetic acid…

A: We don't need to change ka to kb . If you want to change then use the formula  kB= kw/ka   Sodium…

Q: What concentration of NH4Cl is necessary to buffer a 0.50 M NH3 solution at pH = 9.00? (The Kb for…

A: The NH4Cl gives NH4+ and Cl- ions, so the initial concentration of NH4Cl = [NH4+] The buffer…

Q: Carbonic acidhas a Ka of 4.7 x 10-11 for the equation below. H2CO3(aq) co, (aq) 2H* (aq) 0.05 M…

A: The pH of a solution is the negative logarithmic of hydrogen ion concentration in the solution.…

Q: Pyrazolium Chloride is a weak acid (C3H4N2HCl; Ka=1.4x10-3). How many grams of Pyrazole (conjugate…

A: Given: Ka of C3H4N2HCl = 1.4 X 10-3  Concentration of C3H4N2HCl = 0.3 M And pH of buffer solution =…

Q: Sodium hypochlorite (NaOCl, the active ingredient of bleach) was dissolved in a solution buffered to…

A: 1) Solution buffered to pH = 6.20 2) NaOCl as an active bleaching agent pKa=7.518

Q: CH3COO + H2O → CH3COOH + OH- K₂=1.8x10-5(for acetic acid)

A: Given: Concentration of CH3COONa is 0.100 M Given reaction is: CH3COO-+H2O→CH3COOH+OH- Ka is…

Q: Q1//A solution of 0.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A:

Q: How many moles of BHCl (acidic salt) would need to be added to 417 mL of 1.33 M B (a weak base) to…

A:

Q: Calculate the [NH3] in a solution of 0.210 M ammonium fluoride (NH,F). Hint: Use the Ka of HF (6.8 x…

A: We have find out the [NH3] in a solution of 0.210 M ammonium fluoride (NH,F).

Q: - Calculate the acid dissociation constant for a solution of a 0.20M HF if the pH is 4.32.

A: given :- pH of HF solution = 4.32               concentration of HF = 0.20 M  To calculate :-  value…

Q: The PH of a buffer solution containing 0 5mole/litre of CH3COOH and 0.5mole/litre CH3COONa has found…

A: PH of solution after adding the 0.1M HCl is calculated as

Q: 21. calculate the H+ in M for 0.620 M C2H5NH3CI solution. Kb for solution is 5.60•10^-4

A:

Q: A solution of acetic acid is 2.0% dissociated at 25.0°C. What was the original concentration (in M)…

A: I am supposed to answer only one question.

Q: 10. Assuming that the dissociation products are of equal concentration, classify the pH of the…

A:

Q: Calculate the pH of a solution containing 0.20 M HC2H302 and 0.25 M NaC2H3O2. The Ka for HC2H3O2 is…

A: pKa = -log Ka = - log (1.8×10-5) = 4.74

Q: Calculate the ratio of CH3NH2 to CH3NH3CI required to create a buffer with pH = 10.18. Express your…

A: Basic Buffer is a solution in which both base and salt of base is present. Buffer is a solution…

Q: What is the pH of the sodium lactate solution? C3H5O3 + H₂O = HC3H5O3 + OH- [C3H5O3] = 3.22 × 10-¹ M…

A:

Q: Sodium hypochlorite (NaOCl, the active ingredient of all bleaches) was dissolved in a solution…

A: pH of buffer solution is calculated by using Henderson Hassel balch equation

Q: a) Find the pH of 0.087 M NaCN. (Ka for HCN = 6.2  10-10.) b) Find the pH and fraction of…

A: Given,Ka of HCN = 6.2×10-10

Q: alculate the [H+] and the pH of a buffer solution that is 0.20 M in HC2H3O2 and contains sufficient…

A: the solution is as follows:

Q: Calculate the pH after addition of 19.35 mL of 0.1302 M KOH to 25.00 mL of 0.1785 M CH 3CH 2CO 2H. K…

A: Given:  Molarity of KOH is 0.1302M Volume of KOH is 19.35mL Molarity of CH3CH2CO2H is 0.1785M Volume…

Q: What is the pKa of an unknown monoprotic acid solution of 0.0450 M at pH 2.78

A: Given data: pH = 2.78  Molarity of acid solution = 0.045 M Formula used: pKa = -log Ka

Q: I need to find the pH of this weak acid and strong acid solution. I set up an ICE table with the…

A: Dissociation of strong acid such as HNO3 is 100%. Dissociation of weak acid such as HC6H5O is only…

Q: 1. A buffer solution is made from 0.4M CH3COOH and 0.6M CH3COO–. If the acid dissociation constant…

A:

Q: Calculate the [H+] in a solution that is 0.18 M in NaF and 0.25 M in HF. (Ka = 7.2 × 10–4) Group of…

A: Solution, which resist in pH change value upon addition of small amount of strong acid or base (less…

Q: (a) Calculate the percent ionization of 0.125 M lactic acid(Ka = 1.4 x10-4 ). (b) Calculate the…

A: a) The percent ionization of 0.125 M lactic acid has to be given, The equilibrium reaction of acetic…

Q: What is the percent ionization of a 0.1 M monoprotic ?acid solution (Kg = 1.6 x 10-4) at 25°C %3D…

A:

Crystal Structures

Solids are present all around us. They have different properties and applications. Diamond and graphite are two well-known solids. Diamond is the hardest material in the world and is used in making jewelry. Graphite on the other hand is soft. The lead of your pencil is graphite. Why are they so different in appearance and properties despite the fact they are chemically the same? Both are allotropes of carbon. The answer lies in the structure, the way constituent particles are arranged in the solids.