If you mix 350 grams of NACN in 640 ml of water, what is the pH? How many grams of its conjugate acid (HCN), would you need to add to change the pH to 7.85? If I now add 68 ml of 1.6 M HCI, what would the new pH be?

If you mix 350 grams of NACN in 640 ml of water, what is the pH? How many grams of its conjugate acid (HCN), would you need to add to change the pH to 7.85? If I now add 68 ml of 1.6 M HCI, what would the new pH be?

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

SectionU4.22: Drip Drop: Titration

Problem 6E

See similar textbooks

Related questions

Q: Define pH. What pH range is considered acidic? Basic? Neutral? (Assume 25 °C.)

Q: what is the pH of the diluted solution? The

A: We have to find pH of resulting solution

Q: A solution is made by dissolving 35.4 g HBr in 635 mL of water. Calculate the pH of this solution.

A: Given, Mass of HBr =35.4 g Volume of solution = 635 mL = 0.635 L pH of the HBr solution = ? Note:…

Q: What is the pH of a 0.109 M solution of HI? Enter your answer in decimal format with two decimal…

A: Given : Concentration of HI = 0.109 M

Q: A chemist dissolves 631. mg of pure hydrochloric acid in enough water to make up 240. mL of…

A: Given as Mass of HCl=631 mg Volume of solution= 240 mL The pH of the solution has to be calculated.

Q: What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179…

Q: The hydroxide ion concentration of a solution is 6.7 X 10-8. What is the pH level of the solution?…

Q: A chemist dissolves 363. mg of pure hydrochloric acid in enough water to make up 170. mL of…

A: Solution for both questions are

Q: Calculate the pH that results when the following solutions are mixed: 35 mL of 0.20 formic acid, 55…

Q: 8.50g of the strong base, Ba(OH)2, (molar mass = 171.342 g/mol) was dissolved in enough water to…

A: Given that: mass of Ba(OH)2= 8.50 g volume of Ba(OH)2= 500.0 mL = 0.50 L molar mass = 171.342…

Q: (a) When 6.3 g of nitric acid are dissolved in water to produce 500.0 mL of solution, what is the…

A: pH of solution is defined as the concentration of hydronium ion H3O+ present in the solution.

Q: The pH scale was designed to make it convenient to express hydrogen ion concentrations that are…

Q: An aqueous solution has a hydronium ion concentration of 4.0 x 10/ M. What is the pH of this…

A: Answer: pH of a solution is the negative of logarithm of hydronium ion concentration.

Q: The Kb of C6H5NH3+ is 3.98x10-10 The Kb of C6H5NH3+ is 3.98x10-10 What is the [H3O+] concentration…

Q: A chemist dissolves 742. mg of pure hydrochloric acid in enough water to make up 280. mL of…

A: Given : Mass of HCl = 742 mg = 0.742 g…

Q: What is the pH of a solution that has a hydrogen ion concentration of 1.6×10−8 M ?

A: Given :- hydrogen ion concentration i.e. [H+] = 1.6 × 10-8 M To determine :- pH of solution

Q: Classify the following aqueous solutions as strongly acidic, weakly acidic, neutral, weakly basic,…

A: (a) battery acid, pH 0 ----> strongly acidic. (b) lime juice, pH 2.7 -----> strongly acidic.…

Q: A chemist dissolves 846. mg of pure hydrochloric acid in enough water to make up 120. mL of…

Q: Calculate the pH of the solution. Assume 1.0 L of solution. You must identify the type of solution…

Q: The pH of an aqueous solution of 0.325 M hydrocyanic acid is

A: The concentration of hydrocyanic acid (HCN) = 0.325 M Ka of hydrocyanic acid = 6.2×10−10

Q: A sample of TANG juice has a hydronium-ion concentration of 1.7 x 10^-4 M. What is the pH? Is the…

Q: A chemist dissolves 149. mg of pure potassium hydroxide in enough water to make up 110. mL of…

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH is simply…

Q: The pH of a normal rainwater is 5.80. What will be the pH of rainwater that falls near a…

A: pH is negative logerathim of hydrogen ion concentration and is expressed by pH = - log[H+]…

Q: A solution of sodium cyanide, NaCN, has a pH of 11.20. How many grams of NaCN are in 835 mL of a…

Q: Enter your answer in the provided box. A solution of formic acid (HCOOH) has a pH of 2.14. How many…

Q: A. The hydrogen ion concentration of a solution is 6.40x10-12 M. What is the pOH of the solution?…

A: For part A, given the concentration of the hydrogen ion = 6.40x10-12 M. We have to calculate the pOH…

Q: What is the pOH of a solution with a pH of 1.80? The answer should be put to the proper number of…

A: Applying formula PH+POH= 14

Q: Two drops (0.1 mL) of 7.0 M HCl are added to water to make 1.0 L of solution. What is the pH of this…

A: Given: Concentration of HCl initially = 7.0 M Volume of initial HCl taken = 0.1 mL = 0.0001 L…

Q: An aqueous solution contains 0.050 M HCl at 25.0 °C. What is the pH of the solution?

A: The pH of the solution can be calculated as follows -

Q: The hydroxide ion concentration of an aqueous solution of 0.429 M hydroflioric acid is [OH-] =…

A: Please note- As per our company guidelines we are supposed to answer only one question. Kindly…

Q: The pH of an aqueous solution at 25°C was found to be 4.90. The pOH of this solution is . The…

A: We will calculate all parts

Q: What is the pH of a solution prepared by dissolving 1.10 g of solid sodium hydroxide in 815 mL of…

A: pH of a solution is defined as the negative logarithm of H3O+ ion concentration. pH = -log[H3O+]…

Q: K/U Which of the following molecules or ions can act as an acid or a base? Write the two possible…

Q: Calculate the pH of the solution. Assume 1.0 L of solution. You must identify the type of solution…

Q: solution NaOH(aq)NaOH(aq) contains 6.96.9 g NaOH(s)NaOH(s) per 100.0100.0 mL of solution. Calculate…

A: Given that: Mass of NaOH(s) = 6.9 g Volume of solution = 100.0 mL = 0.1 L pH of the solution = ? pOH…

Q: at a certain temperature, the pH of a neutral solution is 7.87. What is the value of Kw at that…

A: We have to calculate the Kw for neutral solution.

Q: What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous…

A: From given pH value pOH is determined. Then, [OH-] concentration is calculated.

Q: What is the pH of the solution? [OH-] = 8.4 x 10-3 M use significiant figures

A: pH is scale from which we determine either the given solution is acidic or basic. The pH scale is…

Q: What is the pH of an aqueous solution made by combining 43.55 mL of a 0.3692 M ammonium chloride…

A: Ammonia, NH3(aq) is a weak base and ammonium chloride, NH4Cl, or NH4+(aq) is a conjugate base of…

Q: What is the pH of a 0.21 M solution of formic acid? __________ What is the degree of ionization of…

A: The reaction of ionization of Formic acid

Q: solution

A: We will calculate H+

Q: What is the pH of a 0.159 M aqueous solution of ammonium perchlorate, NH4ClO4 ? pH = This…

A: Given, Concentration of ammonium perchlorate (NH4ClO4) aqueous solution = 0.159 M

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−][OH−], of 7.69×10−7 M.

A: Calculate the pOH of the solution, pOH =- log [OH-]= - log (7.69 × 10-7)= 6.11

Q: What is the pH of a 0.325 M solution of HI? Enter your answer in decimal format with two decimal…

A: Given : Concentration of HI = 0.325 M Since HI is a strong acid. Hence it will dissociate completely…

Q: Convert the concentration 1 ppm NaCl to mg/L as CaCO3. What is the pH of an aqueous solution that…

A: The concentration of a solution is the amount of solute particles present in the solvent. This can…

Q: solution has a [H+] of 2.5 ×10-3 M. What is the pH of this solution?

Q: please highlight the correct answer

A: The addition of an acid to water decreases the pH of water by introducing hydrogen ions in the…

Q: Determine the pH of a solution a) when 41.5 g of lactic acid is dissolved with water and diluted to…

Question

The following question is asking three parts**

2. If you mix 350 grams of NACN in 640 ml of water, what is the pH? How many grams of its conjugate acid (HCN),
would you need to add to change the pH to 7.85? If I now add 68 ml of 1.6 M HCI, what would the new pH be?

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

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Quality Assurance and Calibration Methods

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

Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.
Acids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.
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?
Use the same symbols as in Question 61 ( = anion, =OH) for the box below. (a) Fill in a similar box (representing one liter of the same solution) after 2 mol of H+ (2) have been added. Indicate whether the resulting solution is an acid, base, or buffer. (b) Follow the directions of part (a) for the resulting solution after 2 mol of OH- (2 ) have been added. (c) Follow the directions of part (a) for the resulting solution after 5 mol of OH- (5 ) have been added. (Hint: Write the equation for the reaction before you draw the results.)
Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2