Indicate the second endpoint for a citric acid titration (H3C6H5O7 Ka1-7.01x10-4, Ka2-1.70x10-5, and Ka3-6.46x10-6) with a strong base. Choose the most suitable indicator to visually determine the second endpoint of this titration. Briefly explain your selection and describe the color change seen. a. Methyl Yellow (pKa=3.50) changes from red to yellow b. Methyl red (pKa=5.00) changes from red to yellow c. Bromophenol Blue (pKa=4.10) changes from yellow to blue d. Bromocresol green (pKa=4.70) changes from yellow to green e. Neutral Red (pKa=7.00) changes from red to yellow

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Q: Calculate the pH during the titration of 40.00 mL of 0.1000 M propanoic acid (HPr; Ka = 1.3x10-5)…

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Q: When using a strong dibasic base (titrant) to titrate a weak monoprotic acid (analyte) at 25°C,

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Q: The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid…

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Q: 60.0 mL of 0.60 M NAOH is titrated using 0.20 M H2SO4. What is the volume of H2SO4 needed to reach…

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Q: Oscar titrates 100.0 mL of 0.50 M hydroxylamine with 1.0 M HI. What volume of HI is needed to reach…

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Q: 1. Based on the shape of the curve, what is the nature of the analyte? Strong acid Strong base Weak…

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A:

Q: Consider Titrating a 50 ml of 0.1M H3A (Given Ka1= 1x10^-4 , Ka2=1x10^-9, Ka3=1x10^-12 ). Calculate…

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Q: 1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NAOH. The results of this titration…

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Q: For the titration of 30.0 mL of 0.300 M NH, with 0.500 M HCl at 25 °C, determine the relative pH at…

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Q: How many milliliters of 0.118 M HCl are needed to titra (a) 48.2 mt of 0.0708 M RbOH 19 72578 Xmt…

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Q: Sodium tetraphenylboron is the titrant for what precipitimetric method?

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A: we have, 20 mL of 1M NaOH 2M of HCOOH ( Ka= 1.8×10-4)

Q: 5. Refer to the figure to answer the questions a & b. a. What is the pKa of the unknown acid?…

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Q: 4. ( You are performing the titration of a buffer with a pKa of 7.2. You start at the pka, and after…

A: A Buffer solution resist the change of pH,When small amount of acids ar base is added.

Q: 2) For this problem, refer to the titration chart below 14.0 12.0 100 8.0 pH 6.0 4.0 2.0 5.0 10.0…

A: The titration curve given is as shown below.

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Q: A stock solution contains 1.4 mM phosphate. From this stock solution, 51.4 uL is diluted with 264 uL…

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Q: Yolanda titrates 40.0 mL of 0.40 M HBrO with 0.10 M LIOH. What volume of lithium hydroxide is needed…

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Q: Calculate the pH at each of the following points in the titration of  100.0 mL of 0.100 M H2A (pKa1…

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Q: Malonic acid is a dicarboxylic acid with structure CH2(COOH)2 with Ka1 1.5 x 10-3 and Ka2 = 2.0 x…

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Q: Prepare a spreadsheet for the titration of 48.2 ml of 0.2025 M H2L with 0.1012 M N2OH, pKa1-3.65 and…

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Q: I did an experiment called Potentiometric Analyses where we titrate NaOH with a solid unknown weak…

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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.