Which of the following substances is more soluble in a hydrochloric acid solution than in a sodium hydroxide solution?   HClO4   MgCl2   NH4NO3   Ni(CH3COO)2   NaI

Q: A mixture needs to be separated to obtain pure individual components. One of the components is a…

A: For separation of mixture, we have to choose a perticular solvent that dissolve that particular…

Q: Which of the following aqueous solutions are good buffer systems? 0.11 M acetic acid + 0.15 M nitric…

A:

Q: 9. Measurement of Acetylcholine Levels by pH Changes You have a 15 mL sample of acetylcholine (a…

A: Given data  15ml volume  PH= 7.65 After decreases PH = 6.87 Find nanomol

Q: A common indicator ionizes in solution according to the equation: HA(aq) + H"(aq) + A (aq) reaction…

A: If excess HCl is added to the solution, the solution turns (yellow) as the (forward) reaction…

Q: Solid aluminum hydroxide and solid aluminum phosphate are in equilibrium with a solution containing…

A: Solution-  The balanced reaction will be- AlPO4 (s) +3NH4OH ⇌ Al(OH)3 (s) + (NH4)3PO4Conc. (NH4)3PO4…

Q: You need to produce a carbonic (H 2 CO3)/bicarbonate buffer solution that has a pH of 4.50. You…

A: Carbonic/bicarbonate buffer solution has a pH of 4.50 . 0.60 L solution contains 0.20 moles of…

Q: An analytical chemist is titrating 179.3 mL of a 0.3400M solution of benzoic acid (HC H₂CO₂) with a…

A: First we need to calculate moles of both compounds and then draw an ICE table for their reaction.…

Q: An analytical chemist is titrating 149.1 mL of a 0.1500M solution of diethylamine ((C₂H₂)₂NH) with a…

A: Solution of diethylamine and HNO3

Q: How many of the following three pairs would make an effective buffer? NaBr/HBr NaCl/HCl NaCHO…

A: Which one is an effective buffer??

Q: the solutions are additive and that Kp = 4.4 x 104 for methylamine.

A: The question is based on the concept of EQUILIBRIUM. we have to calculate pH of the solution…

Q: You found a bottle of aqueous solution in the laboratory cabinet. Unfortunately, the label has been…

A: i) The pH of the solution is 3.00, that means it is an acidic solution. This rules out the solution…

Q: A 0.200 M solution of a weak base has a pH of 9.00. What is the base hydrolysis constant, Kp, for…

A: Given: pH of solution= 9 Concentration of weak base = 0.2 M

Q: Write a net ionic equation for the reaction with OH- by which antimony(III) hydroxide dissolves when…

A: Here we have to write the net ionic equation for the reaction of hydroxide ion with antimony (III)…

Q: Which of the fellowing aqueous solutions are good buffer systems? O0.38 M hypochlorous acid + 0.25 M…

A:

Q: Which of the following aqueous solutions are good buffer systems? | 0.35 M ammonia + 0.30 M sodium…

A: Buffer solutions are the solutions containing a mixture of weak acid and its conjugate base or a…

Q: Which of the following combination of solutions will form a buffer solution?            (A)  50.0…

A: Buffer solution: The solution which contains weak acid mixed up with its conjugated acid or a weak…

Q: What is the pH of a buffer solution containing 1.25 M NH₃ and 0.75 M NH₄NO₃? Note that the base…

A:

Q: What are the hydronium ion concentration and the hydroxide ion concentration in pure water at 25 °C?

A:

Q: Which of the following equal molar salt solutions is expected to have the highest pH? All of these…

A: Given question related to identifying the salt solution which has the highest pH among the given…

Q: You found a bottle of aqueous solution in the laboratory cabinet. Unfortunately, the label has been…

A: i) The pH of the solution is 3.00, that means it is an acidic solution. This rules out the solution…

Q: indicate whether the following salts will be soluble or insoluble in water HgCl BaCO3 SrBr2 and…

A: Given salts-         HgCl   ,   BaCO3  ,   SrBr2  and   ZnSO4We need to write the above salts will…

Q: of the following substances, when added to a solution of Chlorous acid             (HClO2), could…

A: A buffer solution is defined as solution which resistance to change in it's pH value even when small…

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

A: HNO2 is a weak acid. It dissociates as,  HNO2 ⇌ H+ + NO2- So, According to Le Chatelier's Principle,…

Q: Describe what happens when you mix an aqueous solution of NaOH with an aqueous solution Fe(NO3)2? In…

A: An aqueous solution of NaOH mixed with an aqueous solution Fe(NO3)2

Q: For the H₂SO4 and NaOH titration, the endpoint is ideally reached when a green color is observed. If…

A: Given , titration of NaOH and H2SO4

Q: which salt forms a 0.1M aqueous solution with the highest ph?  CaSo4 NH4Br KF NaNO3 FeCl3

A: INTRODUCTION: Neutral solutions with a pH range of 7. Acidic solutions with a pH range of less than…

Q: Which of the following aqueous solutions are good buffer systems? O 0.38 M barium iodide + 0.27 M…

A: Buffer solution formed by combination of weak acid or base with salt of weak acid or base…

Q: the reaction of a strong acid with a strong base produces a salt and another product what is the…

A: We need to determine the products of reaction between strong acid and strong base.

Q: What salt is formed in the acid base neutralization reaction below HBr and Mg(OH)2

A: HBr + Mg(OH)2 --->

Q: Which of the following aqueous solutions are good buffer systems? O 0.13 M hydrocyanic acid + 0.16 M…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: 1) Write the equilibrium constant expression for the dissociation of acetic acid

A: Below attached file showing the details answer. All the best.  As per Bartleby answering guidelines…

Q: Which of the following aqueous solutions are good buffer systems? O 0.22 M perchloric acid +0.24 M…

A:

Q: A chemistry graduate student is given 100. mL of a 1.40M methylamine (CH3NH2) solution. Methylamine…

A: pKb  = - log Kb            =  - log (4.4  * 10-4 )          = 3.36pKa = 14-pKb       = 14- 3.36…

Q: Each of the insoluble salts below are put into 0.10 M hydrobromic acid solution. Do you expect their…

A: when Each of the given insoluble salts below are put into 0.10 M hydrobromic acid solution. silver…

Q: 1. The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10^-5. If 7.285 grams of aniline is…

A: We can easily calculate the equilibrium concentration of the species by constructing an ICE table.…

Q: Formic acid (HCO2H, Ka = 1.8 × 10-4) is the principal component in the venom of stinging ants. What…

A: Volume of formic acid = 25.00 mLVolume of NaOH solution required to reach the equivalence point =…

Q: estion 48 What is the molar solubility of Agl Ksp 8.3 × 101 in the presence of 0.05 M KI? O 9.11 x…

A:

Q: What is the pH of a buffer solution made by adding 0.15 mole of lactic acid HC3H5O3 and 0.12 mole…

A: A buffer is a solution which resists a change in its pH, i.e., its pH does not change. For example,…

Q: A student performs a titration of 31.0 mL of a phosphoric acid (H3PO4) solution of unknown…

A: Given,

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: Order the following salt solutions in terms of their ability to raise the pH value of an aqueous…

A: The objective of the question is to rank the given salt solutions based on their ability to increase…

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.