Consider the following acids:AcidsHC2H3O21.8x10-5HE6.8x10 4HCN6.2x10 10HCIO2.9x10 8 What is the pH of an aqueous solution that consist40.0 mL of 0.050 M HI and 30.0 mL solutioncontaining 0.040 M HC2H3O2.

Mixture of strong and weak acid will release proton. The strong acid will release according to its…

Answered: What is the pH of an aqueous solution…

What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HI and 30.0 mL solution containing 0.040 M HC2H302.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: What is the pH of a solution prepared by mixing 25.0 mL of 0.180 M HC,H30, with 40.0 mL of 0.250 M…

A: pH of the solution = 13.71

Q: What is the pH of a 0.500 mol/L solution of sodium cyanide (NaCN) if the cyanide ion has a K₁ = 1.61…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: What is the pH of a solution prepared by mixing 75.10 mL of 0.02250 M NaOH with 19.22 ml of 0.08780…

A: Given:Volume of NaOH = 75.10 mLMolarity of NaOH = 0.02250 MVolume of HCl = 19.22 mlMolarity of HCl…

Q: 18) How many grams of sodium fluoride (MM =41.988 g/mol) must be added to 250.0 mL of a 0.100 M…

A: This question based on formula of acidic buffer NaF and HF is acidic buffer The answer is c that…

Q: What is the pH of a solution

Q: What is the pH of a solution that is 2.0 M HF and 2.0 M F–? Does your answer make sense?

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: Hydrofluoric acid (HF) has a Ka value of 7.2 x 10-4. What is the pH to 2 decimal places when 6.875…

A: When weak acid HF reacts with KOH to form a buffer solution . The pH of buffer solution can be…

Q: 2. Calculate the pH of a solution that contains 150 mL of 0.25 M NaF and 252 ml of 0.30 M HF. K, =…

A: Given volume of HF is 252 mL and strength is 0.30 M Given volume of NaF is 150 mL and strength is…

Q: What is the pH of a 75.0mL of a 0.1M pyridine (C5H5N) solution (kb = 1.7 x 10 -9) when 100mL of a…

A: Acid and base have equal mole so they neutralise to each other and we get salt. So we will use…

Q: Butyric acid, C3H,COOH, has ionization constant of 1.54 x 105. a) Calculate the pH of 50.0 mL of a…

A: part C pH of the resulting solution can be calculated using the values of volume and molarity of the…

Q: What is the pH of a solution prepared by mixing 18.00 mL of 0.277M CH3COOH with 50.00 mL of 0.166 M…

Q: What is the pH of a solution that contains 0.10 M cyanic acid and 0.20 M sodium cyanate?

Q: How many milliliters of 1.08 M HClO4 should be added to 1.80 g of imidazole to give a pH of 6.993?

A: To calculate the amount of 1.07 M HClO4 required to achieve a specific pH, the reaction of…

Q: What is the pH for a 400 ml solution of 1.6 M Benzoic Acid if you added 175 grams of conjugate base…

A: The solution is given below -

Q: What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HCl and 30.0 mL. solution…

A: pH: It is a scale that determines, whether the given compound or solution in acidic, basic or…

Q: Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: 1.2 g of the strong base NaOH are dissolved in water and diluted to 50.0 mL. What is the pH of this…

A: Mass of NaOH = 1.2 gVolume of solution = 50 mL = 50 mL x 10-3 L/mL = 0.050 L

Q: t is the pH of a 0. M solutI 350 M solution of NaOH is added? The K, of HA is 4.3 x 10-4.

A: We have to tell which option is correct from given choices of options by telling what is the pH of…

Q: Acid dissociation constants for sulfurous acid are given below. Solution A and Solution B are mixed.…

A: Given data,Molarity of KHSO3=1.00MVolume of KHSO3=200mLMolarity of KOH=1.00MVolume of KOH=40mL

Q: Calculate the pH of a solution formed by mixing 200.0 mL of 0.10 M CH3NH2 with 250.0 mL of 0.15 M…

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

Q: NH3 is a weak base (K₁ = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: A solution is given that is 0.036 M in NH4Cl at 25oCKb = 1.8*10-5Need to find the pH

Q: How many moles of NH4Cl must be dissolved in 500. mL of aqueous solution, in order to produce a…

Q: What is the pH of a solution containing 1 mM of a strong acid (e.g., hydrochloric acid)?

A: pH is calculated by using the formulapH= - log [ H+ ] Where [ H+ ] = Hydrogen ion concentration

Q: A chemist must prepare 800.0 mL of nitric acid solution with a pH of 1.00 at 25 °C. He will do this…

A: The volume of the diluted solution of nitric acid is .The pH of the diluted solution of nitric acid…

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: To calctulate the pH, we would use Ka or Kb expression. “Since you have posted multiple questions,…

Q: What is the pH of a 75.0mL of a 0.1M pyridine (C5H5N) solution (kb = 1.7 x 10 -9) when 100mL of a…

A: Go through the image provided

Q: What is the pH of a solution made from combining 2.49 mol (CH3)2NH2Cl and 5.18 mol (CH3)2NH in a…

A: Henderson-Hasselbalch equation explains the relationship between of solution and of acid. For a…

Q: The kb for a certain amine BNH2 is 8.6 × 10-6. Calculate the pH when 79.6 mL of 0.110 M BNH2 have…

A: Given, kb for BNH2 = 8.6 x 10-6 We have 79.6 ml (or 0.0796 L) of 0.110 M (or 0.110 mol/L)BNH2 no.…

Q: 3)CH3NH2 is a weak base (?b = 5.0×10-4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH…

A: Given, Kb of weak base CH3NH2 = 5.0×10–4 And , concentration of CH3NH3NO3 = 0.0450 M .

Q: Calculate the pH of a solution that is 1.00 M HClO and 0.50 M NaClO.

A: NaClO is salt of weak acid HClO and strong base NaOH.Therefore it forms a buffer solution ,whose pH…

Q: en 13.75 mL of a 1.074 M solution of KOH has been added to a 27.5 mL f hydrofluoric acid with a…

A: We will calculate pH

Q: If a buffer solution is 0.200M in a weak acid (?a=9.0×10−5)and 0.550M in its conjugate base, what is…

A: Ka = 9.0 x 10-5 pKa = -log Ka = - log ( 9.0 x 10-5) pKa = 4.046 [Acid] = 0.200 M [Conjugate base]…

Q: NH3 is a weak base (?b=1.8×10−5�b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

Q: NH3 is a weak base (Kb = in NH4Cl at 25 °C? pH = x10 TOOLS 1.8 x 10-5) and so the salt NH4Cl acts as…

A: The objective of the question is to calculate the pH of a solution of NH4Cl, a salt of a weak base…

Q: What is the pH of a solution prepared by mixing exactly 25.0 mL of 0.200 M HC₂H3O2 with 15.0 mL of…

A: Given data The concentration of HC2H3O2 is 0.200 M The volume of HC2H3O2 is 25.0 mL The…

Q: What is the pH of a solution that is 0.28 M in acetic acid, HC2H3O2, and 0.69 M in sodium acetate,…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a solution…

Q: what is the pH

Q: Calculate the pH of a 1L aqueous solution that is0.14 M in HF and 0.19 M in NaF after 0.013 mol of…

A: The solution which can resist the change in the pH of solution upon addition of acid or base is…

Q: Butyric acid, C3H,COOH, has ionization constant of 1.54 x 10. a) Calculate the pH of 50.0 mL of a…

A: We have to predict the pH of acid and salt and pH upon mixing the solution.

Q: To what volume should 100 mL of any weak 0.30 molar monobasic acid (HA) or mono-acidic base (BOH) be…

A: According to the Le Chatelier principle, adding water to equilibrium would cause equilibrium left to…

Q: Please explain. What is the pH of a 0.13 molar solution of NH4Cl. where Kb for NH3 = 1.8 10–5)

Q: Calculate the pH of the following solutions. Give your answers to two significant figures. (a) 0.021…

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

Q: What is the pH of a 0.380 M solution of NACN (Ka of HCN is 4.9 x 1010)?

Q: A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is bubbled into a 0.400 L solution of…

A: To calculate the pH of the resulting solution after adding ammonia () gas to hydrochloric acid (HCl)…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Consider the following acids:
Acids
HC2H3O2
1.8x10-5
HE
6.8x10 4
HCN
6.2x10 10
HCIO
2.9x10 8

What is the pH of an aqueous solution that consist
40.0 mL of 0.050 M HI and 30.0 mL solution
containing 0.040 M HC2H3O2.

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

Calculation

VIEW

Conclusion

VIEW

Step by step

Solved in 3 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

If 50.0mL of 0.100M C6H5COOH (Ka = 6.3 x 10-5) is neutralized by 50.0 mL of 0.100M NaOH, what will the pH of the final solution be?
An analytic chemist is titrating 65.9 mL od 0.4200 M solution of piperidine (C6N10NH) with a 0.8800 M solution of HIO3. The pKb of piperidine is 2.80. Calculate the pH of the base solution after the chemist has added 35.0mL of the HIO3 solution. Round to 2 decimal places
What is the pH of a solution that is 0.33 M CH3NH2 (methylamine) and 0.52 M CH3NH3Cl (methylammonium chloride)? (Assume Kw is 1.0 10-14.)
Calculate the pH of a solution that is prepared by dissolving 0.470 mol of hydrocyanic acid (HCN, K, = 6.17x10 10) and 0.164 mol of acetylsalicylic acid (HC,H¬O4, K,= 3.40×104) in water and diluting to 3.00 L. Also, calculate the equilibrium concentrations of HCN, CN", HC,H¬O4, and C,H¬O,. Do not make an approximation unless the initial acid concentration is greater than 1000 x K. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCN] = M [CN]= M [HC,H;04] =| M [C3H¬O4] = M
Calculate the pH of a solution that is prepared by mixing 25.0 g HC2H3O2 and 25.0 g NaC2H3O2 in 800.0 mL solution (Ka HC2H3O2 = 1.8 x 10-5)
A 25 Celsius aqueous solution is made by adding 2.31 liters of 0.348 M NaNO2 to 3.36 liters of 0.118 HNO2. The Ka of HNO2 is 4.7x10-4. What is the pH of this resultant solution?
Calculate the pH of a solution that is 0.520 MM in pyridine (C5H5NC5H5N) and 0.440 MM in pyridinium chloride (C5H5NHClC5H5NHCl).
Calculate the pH of a solution prepared by dissolving 0.350 mol of benzoic acid (C7H502H) and 0.200 mol of sodium benzoate (NaC7H502) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 x10^-5.
Suppose a weak acid has Ka = 4.0 x 10^-9. which is equivalent to Kb? and why??
Determine the base ionization constant (in x 10-5) of a 0.0925 g sample of a weak 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.
A.) What is the pH of a 6.18×10-2 M aqueous solution of potassium nitrite, KNO2?pH = This solution is acidic basic neutral? B.) What is the pH of a 0.264 M aqueous solution of ammonium bromide, NH4Br ?pH = This solution is acidic basic or neutral? . .
What is the pH of a solution prepared by mixing 45.11 mL of 0.8314 M HCl and 42.03 mL of 0.7261 M NaOH? Please see Mixing strong acid and strong base for assistance. Please note that the starting values in the problem all have 4 significant figures. Depending upon the randomization and how many sig figs are lost during subtraction, there may be more significant figures than students typically input for similar problems.