You want to analyze a cadmium nitrate solution. What massof NaOH is needed to precipitate the Cd2+ ions from 35.0 mLof 0.500 M Cd(NO322 solution?

Q: The following salts were added to a beaker of distilled water: NaCI ENH4)2CO3 Ca(NO3)2 Which of the…

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Q: Q12. Which of the following is soluble in water? A. Fe(NO3)2 B. MGCO3 C. Hg,l2 D. CaS Q13. What…

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Q: The concentration of CO in air is determined by passing a known volume of air through a tube that…

A: Given, Volume of air sample = 4.79 L Volume of Na2S2O3 = 7.17 mL Concentration of Na2S2O3 = 0.00329…

Q: 4. Will a precipitate form when 68.2 mL of 0.587 M K,S mixes with 150.6 mL of 0.980 M AGNO,? Ku for…

A: Ionic product is define as the product of molar concentration present in given solution each raise…

Q: . A compound is known to be NazCO3, NazSO4, NaOH, NaCl, NaC2H302 or NANO3. When a barium nitrate…

A: Given: The possibility of the compound is Na2CO3, Na2SO4, NaOH, NaCl, NaC2H3O2 and NaNO3. When…

Q: How do I start to solve this? I am so confused    What moles of 0.416 M Mg(NO3)3 should be added…

A: Note: Given formula is incorrect: Mg(NO3)3 As charge of Mg is always +2, therefore Correct formula:…

Q: Q13. What volume (mL) of 1.00 M K2Cr,0, is required to completely react with 35.0 mL of 0.500 M FeS…

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Q: 4.) Calculate the solubility product constant, Ksp, for lead(II) chromate Ksp = x 10 13 Hint: enter…

A: We have to calculate the solubility product constant for lead chromate

Q: A solution contains 1.33x10-2 M lead nitrate and 1.17x10-2 M nickel(II) acetate. Solid sodium…

A: “Since you have posted multiple questions, we will provide the solution  only to the first question…

Q: A 50.0 ml solution contains only Na2SO4 (MW 142.04 g/mole).  If 40.0 ml of 0.25 M BaCl2 is needed to…

A: To calculate the number of reactants required for product formation, we must have a balanced…

Q: 125 mL of 0.125 M NaOH aqueous solution and 10.0 mL Choose... of 0.0500 M AGNO3 aqueous solution…

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Q: 3. If you have a solution that is 0.001 M carbonate (CO), to what concent concentration of Ag" be…

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Q: 50.00 mL of a solution containing 0.15 M CH2 (CO2 H)2 and 0.020 M MnSO4  Calculate the mass in g of…

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Q: 1. The Ksp of Ca3(PO4)2  is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−1

A: Since, you have asked multiple questions so we solved first question for you step by step.  You can…

Q: You have a solution of 1M BaCl2 and another of 1M Hg2(NO3)2. If you poured them together, what…

A: 1. In double displacement reaction,  cation of one species easily replaces cation of another species…

Q: 100 mL of 0.320 M AgNO3 is mixed with 100 mL of 0.160 M Na2SO4. How many grams of Ag2SO4 will…

A: Given that,  Volume of 0.320 M AgNO3 solution = 100 ML = 0.1 L Moles of  AgNO3 in 0.1 L = 0.320…

Q: Solubility of CrF3 in water is 0.120 g/L at 25  oC.  What is the molar concentration of F- ion in…

A: When CrF3 dissolves, the following equilibrium is established: CrF3(s) <-------->  Cr3+(aq) +…

Q: A solution contains 1.43x10 M lead nitrate and 5.74x10 M silver acetate. Solid potassium sulfate is…

A: Given that: Concentration of lead nitrate =1.43x10-2 M Concentration of silver acetate =5.74x10-3 M…

Q: A 0.4550-g solid mixture containing CaCl2 is dissolved in water and treated with an excess of…

A: Given information,    0.4550-g solid mixture containing CaCl2 is dissolved in water and treated with…

Q: 0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: What mass of AgCI is precipitated from the reaction of 25.0 mL of 0.100M AgNO3 and excess KCI

A: The objective of this question is to find out the mass of AgCl that is precipitated from the…

Q: 3- Calculate the concentration of PO4 when Ag3PO4 starts to precipitate from a solution that is…

A: Answer: Silver phosphate is a sparingly soluble salt, therefore it can be considered that all of its…

Q: SOLUBLE (aq) - INSOLUBLE (s) – able to be Exceptions cannot be Exceptions dissolved in water…

A: This is inorganic chemistry of soluble and insoluble compounds

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.