A solution is prepared at 25 °C that Is Initlally 0.38M in nitrous acid (HNO,),a weak acid with K=4.5x 10*, and 0.36M In potassium nitrite (KNO,).-4D.Calculate the pH of the solution. Round your answer to 2 decimal places.pHCheckExplanation2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacyhp人->esc&Σ

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A solution Is prepared at 25 °C that Is Initlally 0.38M In nitrous acid (HNO,), a weak acid with K= 4.5x 10, and 0.36M in potassium nitrite (KNO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = |

A solution Is prepared at 25 °C that Is Initlally 0.38M In nitrous acid (HNO,), a weak acid with K= 4.5x 10, and 0.36M in potassium nitrite (KNO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = |

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 60QAP: Consider an aqueous solution of HF. The molar heat of formation for aqueous HF is -320.1 kJ/mol. (a)...

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A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
. 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?
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that ale Lewis acids and accept F- ion (for example, BF3 or SbF5]. Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.
Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a Determine the concentrations of H3O+ and HCOO in this solution. b Determine the H3O+ concentration that would be necessary to decrease the HCOO concentration above by a factor of 10. How many milliliters of 2.00 M HCl would be required to produce this solution? Consider that the solution was made by combining the HCl, the HCOOH, and enough water to make 0.425 L of solution. c Qualitatively, how can you account for the differences in the percentage dissociation of formic acid in parts a and b of this problem?
Using an acetic acid/sodium acetate buffer solution, what ratio of conjugate base to acid will you need to maintain the pH at 5.00? Describe how you would prepare such a solution.
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
A solution is prepared at 25 °C that is initially 0.37M in chloroacetic acid (HCH,CICO,), a weak acid with K= 1.3 × 10 °, and 0.087 M in potassium chloroacetate (KCH,CICO, ). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = Continue Su © 2021 McGraw-Hill Education, All Rights Reserved. Terms of Use
A solution is prepared at 25 °C that is initially 0.37 M in nitrous acid (HNO,), a weak acid with K, = 4.5 × 10 *, and 0.38 M in potassium nitrite (KNO,). -4 %3D Calculate the pH of the solution. Round your answer to 2 decimal places.
Calculate the pH at 25 °C of a 0.30M solution of sodium benzoate (NaC,H,CO,). Note that benzoic acid (HC,H,Co,) is a weak acid with a p K, of 4.20. Round your answer to 1 decimal place. PH = de Explanation Check O 2021 McGraw-Hil Education. All Rights Reserved. Tarms of Use f Privacy Accessiblity 5:13 PM O Type here to search. W 5/8/2021 40 144 prt so delete home end num 8. 6. backspace lock