A student is given the following information about an unknown solution. Dissociates 100% Feels slippery to the touch • pH 13.5 What is the possible classification of the unknown solution? O Strong Acid Weak Base Weak Acid O Strong Base

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

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Q: Each row of the table below describes an aqueous solution at 25 °C. The second column of the table…

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Q: a solution of nitrous acid is titrated with NaOH, calculate the pH when the following percentages of…

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Q: mL

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Q: What is the pH of a saturated solution of Fe(OH),? K,, -4.87×10 17 Be sure your answer has the…

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Q: In which of these solutions will the weak acid, HNO,, ionize less than it does in pure water? 0.15 M…

A: Depression in the degree of dissociation of weak electrolyte in presence of strong electrolytes is…

Q: Selection of suitable indicator or choice of indicator-Define

A: In the quantitative analysis, volumetric titration, the significant pH change occurs near or at the…

Q: 7. Which of the following is not a common pH indicator? O phenolphthalein O distilled water blue…

A: A pH indicator is defined as a chemical compound which is used in mainly qualitative analysis and…

Q: 4. State which of the following species are amphiprotic and write chemical equations illustrating…

A: Amphoteric species are species which behave as base and acid in solution

Q: in titrating 40.0 mL of 0.10 M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: The balanced chemical reaction is  HCl + NaOH ------> NaCl + H2O Number mmoles of HCl = molarity…

Q: The table below shows the measured pH of three salt solutions. Identify any cations or anions that…

A: Understanding the impact of salt solutions on pH is fundamental to comprehending the behavior of…

Q: A 0.4-L unbuffered solution needs the pH adjusted from 10.0 to 3.0. How many microliters of a 7…

A: Given Volume = 0.4 L molarity = 7 M

Q: Solution 1 Number Volume 10.0 9.5 9.0 8.0 6.0 HOAc (mL) Volume NaO Ac (mL) Volume Total (mL)…

A: This is a problem based on acid base concept. We will be using the Henderson's equation to find out…

Q: A 0.307-g sample of an unknown triprotic acid is titrated to the third equivalence point using 35.2…

A: Given : Mass of triprotic acid = 0.307 g Concentration of NaOH = 0.106 M And volume of NaOH solution…

Q: A beaker contains 26.202 mL of a 0.131 M solution of KOH. This is titrated with 13.01 mL of a 0.0425…

A: The solution is given below -

Q: 30.0 mL of a 0.20 M solution of the weak base methylamine is titrated with 0.10 M nitric acid…

A: 30.0 mL of a 0.20 M solution of the weak base methylamine is titrated with 0.10 M nitric acid…

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.