**Orthocresol (C₇H₈O) pH Determination Problem**Orthocresol (C₇H₈O) has a $ K_a = 5.50 \times 10^{-11} $. If 100.0 mL of a 0.5000 M aqueous orthocresol solution is mixed with 100.0 mL of a 0.5000 M aqueous sodium hydroxide solution, the resulting solution will have a pH:- A. =7- B. <7- C. >7- D. Cannot be predicted from the information given**Explanation:**This problem involves the mixing of a weak acid (orthocresol) with a strong base (sodium hydroxide). The $ K_a $ value provided indicates the acid's dissociation in water.**Potential Analysis:**- **Neutralization**: 100.0 mL of 0.5000 M orthocresol and 100.0 mL of 0.5000 M NaOH have equal molar amounts, likely leading to complete neutralization.- **Resulting pH**: After neutralization, the resulting solution typically has a pH determined by the presence of the conjugate base of orthocresol and any leftover hydroxide ions, which usually makes the solution basic (pH > 7).Given these conditions, analyze the information and apply your understanding of acid-base reactions to determine the correct answer.

Write the acid dissociation of orthocresol in aqueous medium: C7 H8OH (aq)+H2O(l)→C7 H8O-(aq) + H3O…

Orthocresol (C7H8OH) has a Ka - 5.50 x 1011. if 100.0 mL of a 0.5000 M aqueous orthocresol solution is mixed with 100.0 mL of 0.5000 M aqueous sodium hydroxide, the resulting solution will have a pH O A. =7 O B. <7 O C. >7 O D. Cannot be predicted from the information given

Orthocresol (C7H8OH) has a Ka - 5.50 x 1011. if 100.0 mL of a 0.5000 M aqueous orthocresol solution is mixed with 100.0 mL of 0.5000 M aqueous sodium hydroxide, the resulting solution will have a pH O A. =7 O B. <7 O C. >7 O D. Cannot be predicted from the information given

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: Explain why the pH of mixture C is the same as the pH of mixture A. Mixtures Conductvity (mA) pH A.…

A: Here we have to explain why the pH of mixture C is the same as the pH of mixture A-

Q: Calculate Ka value for a .200 M solution of hypobromous acid (HBrO) with a hydronium ion…

A: Answer: On adding HBrO in water, its ionization will take place and hydronium ions will be produced…

Q: What is the pH of a 100.0 mL 0.0500m HCN(aq) solution which is mixed with 5.00 mL 0.200 M KOH(aq) ?…

Q: Determine the pH of a 1.0M solution of sodium acetate (NaC2H3O2). Ka = 1.8x10-5 for acetic acid.

A: Dear student, As you have asked multiple question but according to guidelines we will solve first…

Q: In a liter of 0.2F solution of propionic acid, HCSHO2_it has ionization constant of 1.34 x 10,…

Q: A solution is prepared at 25 "C that is initially 0.89M in trimethylamine ((CH), N) a weak acid with…

Q: Calculate the pH of each of the following solutions at 25°C. a. 0.175 M HONH, (Kb = 1.1 × 10-8) pH =…

A: Given, pKb= 1.1×10-8

Q: For the following reaction: Part: 0/2 Part 1 of 2 Ï + Identify the Lewis acid and the Lewis base. O…

A: A Lewis acid is a substance that accepts a pair of electrons. On the other hand, a Lewis base is a…

Q: Calculate the pH at 25 °C of a 0.53M solution of pyridinium chloride (C5H,NHC1). Note that pyridine…

Q: Hypochlorous acid (HOCI) is a weak acid with a Ka = 2.90 x 108. What is the pH of a %3D 0.187M…

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

Q: Complete the reaction H₂SO4 + 2 H₂O mplete ionization of HSO4-¹ What is the pH of a 0.001000 M H₂SO4…

A: ->H2SO4 is strong acid which can dissociate completely into ions H+ and SO42-. Molarity of H2SO4…

Q: Calculate the pH, [H2L*], [HL], [L] for each solution of the amino acid proline (Kal = 1.12 x 102…

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

Q: A solution is prepared at 25oC that is initially 0.42 M in a “X” base, a weak base with Kb =…

A: Since the solution is having base X with concentration 0.42 M and its conjugate acid salt with…

Q: Which of the following aqueous solutions will have the highest pH? 0.1 M CH3COOH = 4.7 0.1 M CuCl2…

A: Answer:Ostwald's dilution law gives us a relation for the value of hydrogen ion concentration in…

Q: Determine the pH of a 0.100 M aqueous solution of NaOcI. Data: pK,[HOCI] = 7.40 А 10.20 B 9.75 C…

A: 1- First we will see the Ka from its pKa : pKa = -log(Ka) -pKa = log(Ka) 10-pKa = Ka Ka =…

Q: You will prepare 5 cuvettes with different concentration of sodium phosphate (Pi) using the stock…

A: For calculating the volume of 1 mM Pi, we use the dilution equation, MstockVstock=MfinalVfinal

Q: 6. Calculate the initíal concentration of a solution of NH, which has a pH= 11.33 and K, = 1.8 x 10.…

Q: Calculate the pH for 0.45 M NaOCI. The K₂ value for HOCI is 3.0 x 10-8. K₁ for OCI = [OH-] = pH =

Q: A solution is prepared at 25 °C that is initially 0.16M in ammonia (NH,), a weak base with K, =1.8 ×…

Q: A solution is made by dissolving 26.5 g of LIC3H5O2 in 500.0 mL of water. Using Kb(C3H5O2) = 7.7 x…

A: Given: The mass of LiC3H5O2 = 26.5 g The volume of the solution = 500.0 mL The Kb of C3H5O2- = 7.7 ×…

Q: Calculate the pH of a solution that contains the following analytical concentrations: a. 0.0400 M in…

A: (a) 0.0400 M NaH2PO4 ka1 = 7.11 x 10-3 ka2 = 6.32 x 10-8 (b) 0.0300 M NaH2AsO4 0.0500 M Na2HAsO4…

Q: Calculate the percent ionization and the pH of the following solution of benzoic acid, HC7H5O2 (Ka =…

Q: A solution of ethylamine (CH3CH₂NH2; K₁ = 4.30 x 10-4) produces a pH = 12.67. What is the %…

Q: α A solution is prepared at 25 °C that is initially 0.90M in chloroacetic acid (HCH2CICO2), a weak…

A: Thank you,Please rate my response.

Q: 2. Determine the pH if I add 0.5 moles of NHẠC1 (s) to a 5 L solution of water. (Note: the Ka of…

Q: mass of NaCH3COO must be dissolved in 400 mL of 0.46 M CH3COOH in order to prepare a solution with…

Q: of A chemist titrates 160.0 mL of a 0.6207M nitrous acid (HNO,) solution with 0.2996M KOH solution…

Q: The concentration of H* (or H3O*) from part A should be 1.02x×10-2 mol L-1. What is the pH of the…

Q: A solution is prepared at 25 °C that is initially 0.17M in ammonia (NH3), a weak base with K = 1.8 ×…

A: Solution that contains weak base (ammonia) and corresponding salt (ammonium chloride) of strong…

Q: Arrange the following solution from lowest pH to highest pH:

A: Acid and base are the chemical compounds which upon adding in water change the pH value accordingly.…

Q: What is the pH of a soluti on prepared by dissolving 3.00 g of the weak acid HA (molar mass = 138.12…

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the…

Q: What is the pH of a solution that initially contains 100. mL of 0.20 M H₂CHO (ascorbic acid) 7.5…

A: The objective of this question is to calculate the pH of a solution containing ascorbic acid and…

Q: What is the pH of a 0.0306 M formate (CHO2-) solution at 25 °C (Ka for HCHO2 = 1.8 × 10-4)? (the…

A: Given data: Concentration= 0.0306M Ka = 1.8 * 10-4 Temperature = 298K

Q: What would the predominant form of the following species be in a solution with a set pH = 12.0? pK =…

A: Find the pI (iso electric point) for the given species . pI =( pKa1 +pKa2 ) / 2 pKa + pKb = 14…

Q: Calculate the pH at 25 °C of a 0.85M solution of potassium acetate (KCH, CO₂). Note that acetic acid…

A: Concept based on the salt hydrolysis. Upon the salt hydrolysis of salt of strong base and weak acid…

Q: A chemist titrates 90.0 mL of a 0.3491M aniline (C6H5NH₂) solution with 0.0636M HBr solution at 25…

A: Information of question

Q: Ka(HCN) = 6.2 x 10-10. Determine the pH of 0.82 M NaCN aqueous solution (3 significant figures).

Q: A solution is prepared at 25 °C that is initially 0.38M in methylamine (CH3NH₂), a weak base with K₁…

A: Given,Molarity of methyl amine ( CH3NH2 ) = 0.38 MMolarity of methyl ammonium bromide ( CH3NH3Br ) =…

Q: 13. Arrange the following solution from lowest pH to highest pH: 0.20 М CH-COОН (К. 3 1.8 х 10-)…

Q: a. 0.155 M HONH, ( Къ 3 1.1 х 10 $) pH = b. 0.155 M HONH3C1 pH = c. pure H20 pH = TIONU and 0 155 M…

A: The question is based on the concept of equilibrium. we have been given a weak base hydroxylamine.…

Q: A solution is prepared at 25 °C that is initially 0.44 M in methylamine (CH, NH,), a weak base with…

A: Methylamine is weak base and Methyl ammonium bromide is its salt.so the solution is buffer solution.…

Q: Calculate the pH of the solution. Ro

Q: What is the pH of a 1.5 x 10² M H;SO, solution? Kai = large Ka2 = 1.2 x 102

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: What is the pH of a 0.10 M solution of phenylamine, C6H§NH2? [K» CsH$NH2 = 4.0 ×10-1º mol L-']

A: weak base are those which does not dissociate completely to furnish the hydroxide ion

Q: HC₂H5O₂ has a K₂ = 1.3 x 10-5. What is the pH of a 0.181M solution of HC3H502?

Q: Determine the quantities shown below for a solution that is 0.0780 M in ethylamine,CH₂CH₂NH₂. The K₂…

Q: Calculate the pH for a 0.5 M nitrous acid (HNO2 ) aqueous solution. Ka= 7.1x10-4

A: The acid dissociation constant ( Ka ) for Nitrous acid is given. Ka= 7.1x10-4 [HNO2] = 0.5 M

Q: Calculate the pH of a solution that us 0.2 M NH3 (Kb=1.8 x 10^-5) and M NH4NO3. Consider the…

A: pH is negative logarithm of concentration of H+

Question

**Orthocresol (C₇H₈O) pH Determination Problem**

Orthocresol (C₇H₈O) has a $ K_a = 5.50 \times 10^{-11} $. If 100.0 mL of a 0.5000 M aqueous orthocresol solution is mixed with 100.0 mL of a 0.5000 M aqueous sodium hydroxide solution, the resulting solution will have a pH:

- A. =7
- B. <7
- C. >7
- D. Cannot be predicted from the information given

**Explanation:**
This problem involves the mixing of a weak acid (orthocresol) with a strong base (sodium hydroxide). The $ K_a $ value provided indicates the acid's dissociation in water.

**Potential Analysis:**
- **Neutralization**: 100.0 mL of 0.5000 M orthocresol and 100.0 mL of 0.5000 M NaOH have equal molar amounts, likely leading to complete neutralization.
- **Resulting pH**: After neutralization, the resulting solution typically has a pH determined by the presence of the conjugate base of orthocresol and any leftover hydroxide ions, which usually makes the solution basic (pH > 7).

Given these conditions, analyze the information and apply your understanding of acid-base reactions to determine the correct answer.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 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

19. Consider the weak acid phenol (C6H5OH), for which Ka = 1.05 ×10-10 in aqueous solutions at 25°C. What is the pH of a 0.850 M aqueous phenol solution at 25°C? A) 4.02 B) 5.02 C) 8.95 D) 9.98 E) none of these
What is the pH of a solution prepared by diluting 195.7 mL of 1.55 M HNO3 (Ka>>1) to a total volume of 8.98L? Please report your answer to 3 sig figs.
8. Dimethylamine (CH3),NH is a weak base with a pKa of 11.0 Calculate the pH of a solution of dimethylamine at 0.10 mol.L-1. b. Calculate the pH of a solution of dimethylamine at 1.0 x 10-² mol.L·'. а.
4 A solution is prepared at 25 °C that is initially 0.29M in nitrous acid (HNO₂), a weak acid with K₁=4.5 × 10 Calculate the pH of the solution. Round your answer to 2 decimal places. pH -0 = X Ś and 0.26M in sodium nitrite (NaNO₂) I
Please help in solving the c and d. Thanks
Help please
6.
This is the structure of the antibiotic flucloxacillin (mw 454, solubility at 25°C = 4.4 x 10-4 M). F CI N -N- OH What would be the minimum pH to which you could formulate your aqueous solution of flucloxacillin (pKa = 2.7) with a concentration of 50 mg per 5 ml at 25°C? O a. 10 b. 6.0 OC. 9.4 d. 4.4 O e. 4.7 "I H -S
Exp. D: Calculate the molar concentrations for the species present in a 1.000 M solution of NaHCO3. HCO,¹ CO3²- Species Approx. Molar Concentration Show calculations: Nat H* 1. Calculate the pH of the sodium bicarbonate solution. OH CO₂
L X Scholarship App X eCovalentActivity.do?locator-assignment-take A q q eq Visited Report - Google X NGLSync Portal X OWLv2 | Online X + Q Use the References to access important values if needed for this question. In the laboratory, a general chemistry student measured the pH of a 0.423 M aqueous solution of pyridine, C5H5N to be 9.412. Use the information she obtained to determine the Kb for this base. Kö(experiment) = Submit Answer Retry Entire Group 9 more group attempts remaining 64°F ^ eq O 21 99+ 40) Up 9:50 PM 5/28/2022
8:43 1 ll 5GE Question 11 of 25 Submit The pH for 0.0715 M solution of CCl,CO2H is 1.40. Determine the value of Ka for CCl,CO2H. 1 2 Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. CCI,CO,H(+ H20(1) =H;0*(aq) +CCl,CO2 (ac Initial (M) Change (M) Equilibrium (M) 5 RESET 0.0715 1.40 -1.40 0.040 -0.040 0.032 -0.032 +x -X 0.0715 + x 0.0715 - 1.40 + x 1.40 - x 0.040 + x 0.0340 - x 0.032 + x 0.032 - x
Calculate K₂ or K from experimental data. The pH of a 9.7x10-2-M solution of phosphoric acid (H3PO4) is measured to be 1.65. Use this information to determine a value of K₂ for phosphoric acid. ? H3PO4(aq) + H₂O(1) H₂PO4 (aq) + H3O+ (aq) Ka =