6. Calculate the number of moles in 123 mL of a 0.242 mol/L ammonium carbonate solution.

Q: How many grams of CaC l 2 should be dissolved in 500.0 mL of waterto make a 0.20M solution of CaC l…

A: Given data contains, Volume of water=500 mL=0.5 L Molarity of the solution is 0.20 M.

Q: 1. Calculate the mass, in grams, of sodium hydroxide needed to prepare 500 mL of approximately 0.1 M…

A: Mole = Molarity × Volume in litre Molar mass NaoH = 39.997g/mol.

Q: 3. Calculate how much 6 M H2SO4 you will need to add to water to make 200 mL of a 1 M H2SO4…

A: Here, we have to calculate the amonut of 6 M H2SO4 that will be needed to prepare 200 mL of a 1 M…

Q: calculate the number of grams of sodium hydroxide that must be added to 1L of water to make 15%…

A: Given% of solution =15%=15100Volume of solution=1L=1000ml

Q: Calculate the number of moles of potassium iodate(V) in 25.0 mL of the solution.

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: Calculate grams of HNO3 in 25.5 mL. of 0.200 M HNO3 solution. HNO3 = 63.00 g/mole

A:

Q: How many grams of ammonium chloride (NH4Cl) are there in 545 mL of a 0.400% (m/v) solution of NH4Cl?

A: Since % (m/v) is defined as the percentage of mass of solute present in 100 mL of solution  i.e %…

Q: What is the concentration of ammonia in a solution made by dissolving 3.75 g of ammonia on 12.0 L of…

A: Molarity: The concentration for solutions is expressed in terms of molarity as follows,

Q: What is the concentration of HCL solution after mixing 500 ml of 0.4m HCL solution with 250ml water

A: V1S1=V2S2 V1= Initial volume V2= Final volume S1= Initial strength S2= Final strength

Q: 1. How many moles of NHẠNO3 are in 335 mL of 0.425M solution? 2. How many moles of MgCl, are present…

A: Using formula of molarity we have calculated number of moles of given problems .

Q: How many grams of sodium hydroxide (NaOH) are required to make 500.0 mL of a 15.4 % (m/v) sodium…

A:

Q: Calculate the number of grams of NaOH needed to make 0.500 L of 0.1 M NaOH solution

A: Solutions are prepared by mixing a small quantity of a substance in a large volume of the solvent.…

Q: Solution of barium chlorate by measuring out 17.1 g of barium chlorate into a 50 volumetric flask…

A: Mass of barium chlorate=17.1 g  Molar mass of barium chlorate = 304.23 g/mol Moles = Mass ÷  Molar…

Q: What volume of 9 M HCl must be used to prepare 1.5 L of 0.25 M HCl?

A: The volume of 9 M HCl that must be used to prepare 1.5 L of 0.25 M HCl is to be determined.

Q: 1. Determine the number of grams of NaHCO; that are in 1.2L of a 3.2 M solution

A:

Q: What is the difference between a 1 M solution and a 1 m solution?

A:

Q: how many g of sodium hydroxide are present in 831 mL of a 0.750 M solution

A:

Q: Calculate the amount of conc. HCl

A:

Q: What volume of 0.125 M HCl can be made from 25.0 mL of 12 M HCl?

A: Given data,Molarity of stock solution(M1)=12MVolume of stock solution(V1)=25.0mLMolarity of diluted…

Q: Amount of HCl in grams in preparing 25% 2 liters of solution

A:

Q: Calculate the number of moles of sulfuric acid that is contained in 0.250 Litros of 2 M sulfuric…

A:

Q: Calculate the molarity of a 5-L solution that is formed by adding a 2.6 g of HCl in a certain amount…

A: The molarity is given as the no of moles of solute present in the total volume of solution in the…

Q: c) To what volume should 50.0mL of a 6.00M HCl stock solution be diluted to obtain a 1.50M HCl…

A: Since you have asked multiple question, we will solve the first question for you. If you want…

Q: How many grams of hydrogen chloride are in 50.0 mL of concentrated (12.0 M) HCl solution?…

A:

Q: How many grams of Zn(NO3)2 are in 4.0 L of a 0.55 M solution

A:

Q: Calculate mass of solid NaOH necessary to prepare 1.0 L of 0.10 M NaOH solution.

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: How many moles of HCl and NaOH  are there? 25.00 ml of 0.500 M HCl neutralized 35.0 ml of NaOH…

A: Since HCl and NaOH are strong acid and strong base respectively so they will completely ionized.

Q: 5. Calculate the number of moles of NaCl contained in 0.230L of a 1.8M solution.

A: Applying formula Mole= Molarity× Volume in L

Q: What volume of 1.2M solution will have 8.4g of nitric acid?

A: Molarity is defined as the number of moles of the solute divided by the volume of the solution in…

Q: Calculate the number of grams of NaOH needed to make 1500. mL of a 0.200 M solution.

A: The relationship between moles and molarity is given by,

Q: 12 - How many mL of 2.0 M hydrochloric acid would be required to prepare 200.0 mL of 1.0 M HCI?

A: Molarity of a solution is defined as the number of moles of the solute present per litre of the…

Q: How many grams of sodium chloride are required to make 2.00 L of a solution with a concentration of…

A: Molarity =0.100M Volume = 2L

Q: How many grams of potassium sulfate must be added to make 250ml of a 0.100M potassium sulfate…

A: From given molarity value and volume the moles of potassium sulfate required is first calculated.

Q: 5. Describe how 100 mL of a 0.10 mol/L NaOH solution would be made.

A: The formula to calculate Moralrity (M):   M= no.of moles/ Volume (in liters)   so, substituting in…

Q: How many grams of solid NaCl should be added to a final volume of 100ml to give a 1M solution of…

A: We will use molarity formula to calculate moles of NaCl, then convert it to grams.

Q: Calculate the morality of a solution prepared by dissolving 11.5g of solid NaOH in enough water to…

A: Molarity is defined as  Molarity = moles of solute / volume of solution in L  Volume of solution…

Q: in the preparation of solution, what mL of 0.9% NaCl must be added to make a 100mL solution

A: Given that, % of NaCl= 0.9% Volume of solution= 100 mL Then,

Q: Calculate the volume of a 0.95M NaOH solution needed to prepare 25.0 mL of 0.48M NaOH solution

A: Molarity of NaOH ,M1 = 0.48M Volume of NaOH,V1 = 25.0mL Molarity of NaOH ,M2 = 0.95M Volume of…

Q: What volume of 0.25 M HCl must be diluted to prepare 0.96 L of 2.0×10-²M HCl? L

A:

Q: How many grams of sodium hydroxide are needed to prepare 0.5 liters of a 6.0 M NaOH solution?

A:

Q: Calculate the number of moles of HCl in 1.0 mL of a 0.10 M HCl solution

A:

Q: if there is 19.7 mL of 1.7 M solution of lithium hydroxide used to prepare a solution with a…

A:

Q: What volume of 0.25 M HCl must be diluted to prepare 1.4 L of 7.0×10-2M HCl? _________ L

A: Molarity of a solution is used to express the concentration of the unknown solution. It can be…

Q: What will be the number of moles of HCl in 100 ml of 0.1 M HCl solution?

A: The molarity of a solution is the ratio between the number of moles of the compound to the volume of…

Q: How many moles of HCl are in 250. mL of 0.100 M HCl?

A: Given information,      Volume of HCl solution is 250 mL.      Concentration of HCl solution is…

Q: You want 13.0 L of 1.25 M HCl and have 16.0M HCl. How many liters of HCl would you use to create…

A: Given,  For preparation of 13.0 L of 1.25 M HCl from16.0M HCl. The volume of HCl in liters would you…

Q: How many grams per millilitre of NaCl are contained in a 0.250M solution .

A: We know , Molarity of NaCl = Moles of NaCl / volume of solution in L By using this we can calculate…

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.