**Question:**1 M NaOH has the same pH as 1 M NH₄OH.- ☐ True- ☐ False**Explanation:**This question is asking whether a 1 M solution of sodium hydroxide (NaOH) has the same pH as a 1 M solution of ammonium hydroxide (NH₄OH). NaOH is a strong base, which dissociates completely in water, resulting in a high pH. In contrast, NH₄OH is a weak base, which does not dissociate completely, leading to a lower pH compared to a strong base at the same concentration. Therefore, the pH of 1 M NaOH would be significantly higher than that of 1 M NH₄OH.

pH is the negative logarithm of [H+]

Answered: 1 M NaOH has the same pH as 1 M NH4OH.…

Science

Chemistry

1 M NaOH has the same pH as 1 M NH4OH. O True O False

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: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

Q: What is the pH of 0.055 M KOH solution? What is the pH of 0.55 M KOH solution What is the pH of a…

A: 1. Concentration of KOH = 0.55 M2. Concentration of Chloroacetic acid = 2 M3. Concentration of…

Q: Which of following solutions is a basic solution? A solution with [OH] = 1.7 x 104 M A solution with…

A: On a scale of pH meter , any solution is described as basic in nature if and only if , pH is…

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

A: According to Bronsted-Lowry concept Acid is a species which can donate proton and forms its…

Q: Calculate the [OH- and the pH of a solution with an [H*] = = 6.8 x 10-10 M at 25 °C. [OH]= %3D pH =…

A: The answer to the given three questions can be answered as follows -

Q: Consider an unknown solution. Tests were conducted and the following results were obtained. Red…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

A: Conjugate acid contain one more hydrogen atom and one more positive charge than the base that formed…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: Benzoic acid, HC6H5CO₂, is a monoprotic acid (only one H* ionizes) with a K₂ = 6.5 x 10-5. Calculate…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: There are several theories to explain the compound as an acid or a base.Arrhenius theory is one such…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: 0-7 = acidic 7-14= basic 7 = neutral

Q: The pH of an aqueous solution that is 2.7 x 103 M HCI is . What is the pOH? Circle one: ACID or BASE…

A: Formulas :

Q: Which of the following solutions is acidic? O [H3O+] = 1.0 x 10-7 M O [H3O¹] = 1.5 x 10-1⁰ M O…

Q: Indicate whether the solution is acidic, basic or neutral. Solution pH = 2.4 pH = 9.1 pOH = 6.5 pOH…

A: Introduction To determine whether a solution is acidic, basic, or neutral, we can look at the pH,…

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

A: According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

Q: NaOH is an example of a strong acid. O True O False

A: The strong acids are the ones that are completely dissociated into the water and lose protons or H+…

Q: Classify each aqueous solution as acidic, basic, or neutral at 25 °C. pH = 12.23 Acidic [H+] = 9.1 x…

A: pH: pH can be defined as the negative logarithm of hydronium ion concentration.pH = -log[H+] pH +…

Q: When an acid is mixed with a base, it is neutralized. OTrue O False

A: The given statement is True.

Q: What is the pH of a solution when [-OH] = 10-12 M? Group of answer choices pH = 0 pH = 2 pH = 10 pH…

Q: Ascorbic acid (vitamin C) is a diprotic acid, H2CgHg06. Calculate [H*], pH, and [C&H,0,²] in a 0.12…

Q: Monochloroacetic acid, HC₂H₂ClO₂, is a skin irritant that is used in "chemical peels" intended to…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

Q: If the conjugate acid of a pair is chlorous acid, then what is the name of the conjugate base? O…

A: given that, chlorous acid is a conjugate acid.

Q: H NO3 HF K" H* OH OH K OH F NO3 H* 4* HF OH H* NO3 он K* HF HF Mg(OH) a b Which beaker depicts a…

A: Arrhenius gave the definition of an acid and base. According to him, acids are those substances…

Q: In addition to your recorded pH called make a table showing the corresponding [H3O+]values. Also…

A: We use the below formula to find [H3O+] from pH. [H3O+] = 10-pH

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

Q: Which solution below has the highest concentration of hydroxide ions? pH = 8.2 pH = 5.6 pH = 3.7 pH…

Q: A solution is made by dissolving 13.9 g of HONH:CIO3 in 500.0 mL of water. Does HONH3* have any…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: Fill in the missing chemical formulae in the tables below. acid conjugate base base conjugate acid…

A: 1.acid conjugate basebaseconjugate acidH2OOH-H2OH3O+HClCl-SO42-HSO4−H3O+H2OOH-H2O…

Q: The compound HA is an acid that is soluble in water. Which of the "beakers" below shows HA behaving…

Q: propanoic acid, a weak monoprotic acid (HC3H5O2, Ka = 1.3 x 10-5), calculate [H+] and pH of a 0.10 M

Q: Identify each acid/base as either strong or weak. HCl HC2H3O2 HNO3 H2SO4…

A: Identify each acid/base as either strong or weak. HCl --> strong acid…

Q: Calculate the pH of a 0.53 M HONH2 solution. Give your answer to two decimal places Kb(HONH2) = 1.0…

Q: Carbonic acid, H2CO3, is a diprotic acid. Calculate the concentration of all species (H2CO3, HCO3-…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

A: A conjugate base is a substance that is formed when the original compound donates the H+ ion to it.

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

Expert Solution

Step 1: What is pH?

pH is the negative logarithm of [H⁺]

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

What is the pH of 1.5M NaOH? pH = 12.5 pH-0.18 pH = 14.88 pH = 14.18 MONTRES A
Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Incorrect Acidic pH = 4.57 pOH = 4.97 pOH = 9.52 [H+] = = 9.8 x 10-5 Basic pH = 9.45 [H+] = 5.5 x 10-¹¹ [OH-] = 4.9 × 10-¹1 [OH-] = 5.4 x 10-² Answer Bank Neutral [H+] = 1.0 x 10-7 pOH = 7.00
What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? What is the concentration of hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? M OH- What is the concentration of hydrogen ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? M H+
Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral pH = 3.53 pH = = 12.01 %3D [H* : = 1.1 × 10–6 H+] = 5.2 x 10-10 РОН 3D = 2.59 [OH] = 9.4 x 10-9 РОН 3D 12.04 [H* = 1.0 × 10-7 [OH] = 7.5 x 10-6 РОН — 7.00
Which of the following are strong acids? HI HNO 3 HE HBr
Table 1: Concentrations of [H3O*] and [OH-] when various amounts hydrochloric acid (HCl, strong acid) or hypochlorous acid (HOC1, weak acid) are dissolved in water to make 1.00 L of solution at 25 Moles of acid added 0.00 0.30 mol HCI 0.75 mol HCI 1.00 mol HCI 0.30 mol HOCI 0.75 mol HOCI 1.00 mol HOCI - 1 - [H3O+] (M) 1.0 x 10-7 0.30 0.75 1.00 9.3 x 10-5 1.5 x 10-4 1.7 x 10-4 [OH-] (M) 1.0 x 10-7 3.3 x 10-¹4 1.3 x 10-14 1.0 x 10-¹4 1.1 x 10-10 6.8 x 10-11 5.9 x 10-11 1. For the strong acid, HCl, in model 1, why are there no HCl molecules present in the beaker? 2. For the weak acid in model 1, why are there mostly HA molecules present in the beaker? 3. From Table 1, what happens to [H3O*] as the number of moles of HOCI increases? 4. From Table 1, how are each of the entries for [OH-] related to the corresponding entries for [H3O+]? 5. If you hadn't been told that HOCI is a weak acid, how could you deduce that from Table 1?
Complete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C. conjugate acid conjugate base formula K a -5 HCH3CO₂ 1.8 × 10 HF 6.8 × 10 4 formula K₁₁ ☐ -7 CIO 3.3 x 10 x10
Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral pH = 3.64 pH = 13.41 [OH-] = 9.3 x 10-8 pOH = 4.73 pOH = 12.12 [H+]=1.0 x 10-7 [H+] = 2.9 × 10-10 [H+]=4.0 x 10-4 [OH-] = 1.4 x 10-3 pOH = 7.00 Answer Bank
Ph c) Ph 0= + hy Ph——CH
Complete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C. conjugate acid conjugate base x10 K, formula formula H,CO, 4.5 x 10 10 NH4 5.6 x 10 7 Clo 3.3 x 10