Interpretation:
The relation that
Concept Information:
Acid ionization constant
The equilibrium expression for the reaction
Where,
Autoionization of water:
The equation of equilibrium for autoionization of water is,
The equilibrium expression for water at
Taking negative logarithm on both sides, we get
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Chapter 16 Solutions
CHEMISTRY:ATOMS FIRST (LL)>CUSTOM PKG.<
- 4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong base) is added? Fill in the table. Give your answers with 2 decimals. Initial pH Final pH after adding NaOH Solution (a) 100.0 ml water (b) (c) 100.0 mL 0.150 M HNO2 (a weak acid) (Given: Ka = 4.5 × 10-4) 100.0 mL solution of 0.150 M HNO2 and 0.100 M NaNO₂arrow_forwardWhat is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M? A 34.1 % (NH4 )2SO4 (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) NEED HELP ASAP NO WORK NEEDEDarrow_forward3.134 grams of potassium sorbate (KCH3(CH,)4CO2 ) is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO, is added dropwise to this solution from a burette. Given: K, (sorbic acid) = 1.7 x 10-5. Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above.arrow_forward
- D Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. Note: Solution 1 (Choose one) 2 = H₂O Explanation Solution 3 (Choose one) ▼ W S ▼ Check 3 747 E D (Choose one) Solution 2 $ (Choose one) 4 Solution 4 R % 5 T X 80 G 6 3 MacBook Pro Y & 7 H © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A U 8 J 1 ( 9 ➡ K ) O O P Oarrow_forwardDetermine the pH of each of the following two-component solutions at 298 KK. PART A: 4.5×10−2 M KOH and 2.0×10−2 M Ba(OH)2 PART B: 0.265 M NH4NO3 and 0.105 M HCN PART C: 7.5×10−2 M RbOH and 0.120 M NaHCO3 PART D: 8.8×10−2 M HClO4 and 2.0×10−2 M KOH PART E: 0.120 M NaClO and 5.00×10−2 M KI please answer type in word don't image upload thank you.arrow_forwardCalculate pH and pOH for each of the following solutions and determine whether thesolution is acidic, basic or neutral:(i) [H3O+] = 4.1 x 10-10 M (ii) [OH–] = 7.6 x 10-3 M(iii) [OH–] = 6.9 x 10-4 M (iv) [H3O+] = 3.5 x 10-6 Marrow_forward
- 1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?arrow_forwardA 0.050 M solution of the salt NaA has a pH of 9.00. Determine the [OH] and the pH of a 0.010 M solution of the acid HA. Show your work in the question parts below. Determine the equilibrium concentration of H3O* using the acid ionization equation. Recall that [OH] = 1.0 x 10-5. Consider the ionization equation described below.. HA(aq) + H20(1) =H;O*(aq) + A (aq) 1 Based on the given information, set up the ICE table in order to determine the unknown equilibrium concentration of all reactants and products. НА(ag) H20(1) H;O*(aq) А (ag) + Initial () Change () Equilibrium () 5 RESET 0.010 0.050 +x -2х +2x -x 0.010 + x 0.010 - x 0.050 + x 0.050 - x 0.010 + 2x 0.010 - 2x 0.050 + 2x 0.050 - 2xarrow_forwardThe active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10^–8. (a) The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.arrow_forward
- Part A Water ionizes by the equation H2Ó(1) = H (ag) + OH (ag) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H+] and [OH-]: What is the H+ concentration for an aqueous solution with pOH = 3.10 at 25 °C? Express your answer to two significant figures and include the appropriate units. Kw = [H*][OH ] • View Available Hint(s) Keep in mind that, like all equilibrium constants, the value of K, changes with temperature. ? [H+] = Value Units Submit Part B Arrange the following aqueous solutions, all at 25 °C, in order of decreasing acidity. Rank from most acidic to most basic. To rank items as equivalent, overlap them. • View Available Hint(s) Reset Help РОН — 8.55 0.0023 mol L1 HC1PH = 5.45 0.0018 mol L KOH Most acidic Most basic O The correct ranking cannot be determined. Submitarrow_forwardMethanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 3) A 35.0 mL sample of (monoprotic) lactic acid, C3H6O3, is titrated with 20.0 mL of a 4.0 x 10-4 mol/L sodium hydroxide solution. What is the pH of the resulting solution at the equivalence point, if Ka for lactic acid is 1.4 x 10-4? PLEASE HELP THIS IS VERY URGENTarrow_forward1) Calculate the pH of a solution prepared by dissolving 1.90 g of sodium acetate, CH,COONA, in 64.0 mL of 0.15 Macetic acid, CH;COOH(ag). Assume the volume change upon dissolving the sodium acetate is negligible. K, of CHCOOH is 1.75 x 105. Calculate the amount of heat released or absorbed by the following substance: 90.23g of iron, AT= 86°C Calculate the amount of heat released or absorbed by the following substance: 7.45g of silicon, final temperature = -10°C, initial temperature = 25°Carrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
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