Compare the solubility of zinc sulfide in each of the following aque

Q: *WRITE RESULTS AND DISCUSSIONS OF TITRATION- CONCENTRATION OF VINEGAR *WRITE CONCLUSION

A: A question based on acid-base titrations that is to be accomplished.

Q: 1. A 0.0450 M Ca(X)₂ has a pH of 11.079. Ca(X)₂ is composed of a Ca2+ cation and an unknown anion…

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Q: . Why do we need to correct for the indicator? . What is/are the pairs that cannot exist together in…

A: (i) We need to perform double indicator titration when the experiments is needed to determine and…

Q: When two reactants have combined in proportions and the both of them have been consumed and neither…

A: In the titration the point where the indicator changes color is known as the endpoint. The point…

Q: If your lab partner misread the concentration of the sodium hydroxide solution and recorded a number…

A: Given: Lab partner misread the concentration of NaOH solution and recorded a number that was too…

Q: a. 10.0ml, 0.10M CH3NH2 and 2.5ml, 0.60M CH3NH3(+) CI(-) b. 10.0ml, 0.15M HNO3 and 2.5ml, 0.40M…

A: Here we have to predict which of the following given solutions are not able to form buffer…

Q: Which theory or concept can explain buffer solution precisely? Explain your answer.

A: a buffer solution is formed by mixture of weak acid and its conjugate base or weak base and its…

Q: Determine if true or false: 1) ionic compounds, that dissolve well in water, and strong acids are…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: In a salt that exhibits an exothermic reaction upon dissolution, increasing the temperature will…

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Q: pH of solution in flask 12.0 10.0 8.0 6.0 4.0 2.0 Indicator methyl orange methyl red A 25.0 mL…

A: Answer: Indicator is the chemical substance that indicates about the completion of titration by…

Q: A. [Fe] = 0.012 M, [OH]= 0.015 M, Ksp = 2.5 x 1039. B. [Pb2*1 = 0.060 M, [CI]= 0.034 M, Ksp = 1.6 x…

A: The condition of precipitation is: Ionic product should be greater than the solubility product.

Q: The maximum amount of iron(II) sulfide that will dissolve in a 0.166 M ammonium sulfide solution is

A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…

Q: Give a example of an acid base titration with the equation other than naoh and hcl

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Q: . What willI be the pH if 75 ml 1.0 M HCI is added to 100 mL of 1.0M NAOH?

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

Q: In titrating 40.0 mL of 0.10 M of HCl solution with 0.15 M of KOH „solution what would be the pH of…

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Q: How do I find the moles excess HCl titrated and Moles HCl absorbed by Tablet

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Q: titration

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Q: Is silver bromide soluble or insoluble

A: A compound is said to be soluble in a solvent if it is easily dissolved in it upto a particular…

Q: Which of the following combinations of chemicals makes a buffer? Mark all that apply. (Identifying…

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Q: State any four requirements for successful volumetric titration.

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Q: Consider the reaction of a 20.0 mL of 0.220 M CSH§NHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.241 M…

A: The complete reaction is: C5H5NHCl+CsOH→CsC5H5NCl+H2O

Q: Which of the following aqueous solutions are good buffer systems? 0.15 M barium hydroxide + 0.29 M…

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Q: A 0.229 g sample of impure NaOH requires 16.0 mL of 0.2050 M HCl for neutralization. What is the…

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Q: Comment on the shape of your graph. Thoroughly explain the chemical cause of each flat or steep…

A: The titration curve is a graph of the volume of titrant,  plotted against the pH.

Q: Which of the following aqueous solutions will or will not act as a buffer solution? NaH₂PO4 Mg(NO₂)2…

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Q: The pH of buffer solution depends on the concentration of-

A: A buffer solution resists changes in pH. pH <7 has an acidic buffer solution; pH>7 has a basic…

Q: 0.251 g sample of impure NaOH requires 17.6 mL of 0.2903 M HCl for neutralization. What is the…

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Q: Which one of the following pairs cannot be mixed together to form a buffer solution? HONH2, HONH3CI…

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Q: How do i solve for the precipitates?

A: The solubility rules as follows,

Q: A chemistry student adds a known amount of solution of known concentration to determine the…

A: In acid-base titration, concentration of an unknown acid/base is determined by adding a base/acid of…

Q: A buffer solution is prepared which is 0.110 M both in formic acid (HCO2H) and in sodium formate…

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Q: What factor governs the selection of an indicator for a neutralization titration? A) the final…

A: Indicator are used in acid base titration or neutralization titration to detect the end point of…

Q: In a titration involving sodium hydroxide and hydrochloric acid, if significantly less acid were…

A: We use M1V1 = M2V2 for the determination of concentration of acid or base in the titration method.

Q: What is the final HCl concentration of 66.4 mL of 8.08 M solution diluted to 1.53 L? .351M 3.51M…

A: Given: Initial molarity (M1) of HCl= 8.08 M Initial volume (V1) of solution = 66.4 mL Final volume…

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.