Latent Heat of Fusion of Ice Weight of calorimeter Weight of calorimeter + Warm Water Weight of Warm Water Initial Temperature of Warm Water Weight of calorimeter + Warm Water+ ice Weight of ice alone Final Temperature of Warm Water + ice Latent Heat of Fusion of Ice ( Experimental) Latent Heat of Fusion of Ice ( Theoretical Percent Error 242.1 344.0 40.1 354.0 34.01

Q: How can a substance, like water, show its amphiprotic nature?  What information can be derived from…

A: Water is a solvent with the pH value =7. Water is neutral and a polar protic solvent. The answer for…

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Q: Ampholytes show both acidic and basic properties. In a chart, show schematic how  the solubility of…

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Q: Which of the following anions act as weak bases in solution? Check all that apply. C103 NO₂ CN- CIT

A: Answer:Any specie that loses H+ ion its solution is called Bronsted-Lowry acid and specie forms…

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Q: [1,0] solution pH x1 0.0027 mol/L A O mol/L B 7.03 10 mol/L 4.0 X 10 C

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Q: The "concentration" of water is 55.5M. Calculate percent ionziation.

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Q: You mix 178 moles of phosphoric acid with 123 moles of KOH. Calculate the pH of your solution (note…

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Q: Calculate the pH of a solution that has pH= as [H₂0*]=6.4 × 10² N M. Round your answer to 2 decimal…

A: Given data : [H3O+] = 6.4 * 10-2 M  Now , we use following formula to calculate pH of  a given…

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Q: Within the pH ranges below, where would you expect to exclusively find an basic solution?   4.0 -…

A: pH is negative logarithm of concentration of H+ions. As we know pH range is 0-14.

Q: Plot the trend of graphs while titrating between mixture of strong acid and week acid VS strong…

A: The titration of mixture of strong and weak acid VS strong base is done by conductometric titration…

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Q: If the pH of a solution decreases by exactly two units (e.g. from pH=3 to pH=1), then the ratio of…

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Q: A student is asked to describe the characteristics of the two solutions above, which have the same…

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Q: Normally, the volume of gastric acid in the human stomach ranges from 20. mL to 100. mL and a pH…

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Q: example(s) of an acidic solution(s) that have a measurable alkalinty value? Just some names of the…

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Q: What is the pH of a 6.23x10-3 M aqueous solution of hydrochloric acid?

A: HCl is strong acid hence it dissociated fully in aqueous solution

Q: [H*] 7 4x10-3

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Q: 1 mL of 3.5 M HCI is used to titrate 6.6 mL of NH3 its endpoint. What is the initial molar…

A: Given : Volume of HCl = 1 mL Molarity of HCl = 3.5 M Volume of NH3 = 6.6 mL

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Q: Calculate the pH of 1.055% (by mass) HCl (MM=36.46) solution. Assume density of the solution is…

A: Mass=1.055% Density =1.010 g/ml

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Q: Define normality (i.e., equivalent ion concentrations) for acids and bases, and the relationship…

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A: The following compound are recognized as acidic basic as per follow.

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Q: In which of the following solutions will hydrochloric acid ionize less than in pure water?…

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Q: Practice Exercise Cakulate he standard fre-anergy changes for heflwing frextions at 25C:

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A: The answer is as follows:

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

A: Given,pOH = 3.22 , [ OH- ] = 9.3 x 10-6 ,  pOH = 7.00,  [ OH- ] = 9.7 x 10-9 , pH = 10.91, [ H+ ] =…

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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.