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How many grams of solid K2CO3 are needed to prepare 150. ml of 0.50 by volume K2CO3 solution?
To prepare a 0.50 by volume (v/v) K2CO3 solution, you need 0.50 liters of K2CO3 per 100 mL of solution. For 150 mL, this means you need 0.75 mL of K2CO3. The density of K2CO3 is approximately 2.43 g/cm³. Therefore, the mass of K2CO3 needed is calculated as follows: 0.75 mL × 2.43 g/mL = 1.83 grams.
What else can I help you with?
What mass of K2CO3 is needed to prepare 200 mL of a solution having a potassium ion concentration of 0.150 M?
To calculate the mass of K2CO3 needed, first convert 200 mL to liters (0.2 L). Then, determine the moles of potassium ions needed using the concentration (0.150 M) and volume (0.2 L) of the solution. Since each formula unit of K2CO3 contains 2 moles of potassium ions, you can then calculate the mass of K2CO3 needed using its molar mass.
How much K2CO3 in 10 percent solution?
To determine the amount of K2CO3 in a 10% solution, you need to know the total volume of the solution. For example, if you have 1000 mL (1 liter) of the 10% solution, it means there are 100 grams of K2CO3 in that solution. This is because 10% of 1000 mL is 100 grams.
What volume of 6.0 M HCl is required to react with 10.0 grams of K2CO3?
First, calculate the number of moles of K2CO3 in 10.0 grams. Next, write and balance the chemical equation for the reaction between HCl and K2CO3. Use the stoichiometry of the balanced equation to determine the number of moles of HCl required to react with the moles of K2CO3. Finally, use the molarity of the HCl solution to calculate the volume needed.
What volume of 0.55m nino32 will react with 45ml of 1.50m k2co3 to form nico3and kno3?
To determine the volume of NiNO32 needed to react with 45 mL of K2CO3, you need to use the stoichiometry of the reaction. First, write and balance the chemical equation for the reaction. Then, use the molarity of K2CO3 to calculate the moles of K2CO3 present. Finally, use the balanced equation to find the volume of NiNO32 needed based on the stoichiometry of the reaction.
How many ions are present in 30.0 mL of 0.600 M K2CO3 solution?
There are 3 ions present in K2CO3: 2 K+ ions and 1 CO3^2- ion. To calculate the total number of ions in 30.0 mL of 0.600 M K2CO3 solution, first determine the number of moles of K2CO3 using the molarity and volume. Then, use the stoichiometry to find the number of ions produced per mole of K2CO3.
What is the concentration of K plus ions in a 0.025 M K2CO3 solution assuming complete dissociation?
The concentration of K+ ions in a 0.025 M K2CO3 solution would be 0.050 M because each formula unit of K2CO3 produces two K+ ions when it dissociates completely in solution.
How do you prepare 20 mL of 1.0 M K2CO3 from solid potassium carbonate?
To prepare 20 mL of 1.0 M K2CO3 solution from solid potassium carbonate, you would need to weigh out 3.66 grams of potassium carbonate (molar mass of K2CO3 = 138.21 g/mol), dissolve it in enough water to make a total volume of 20 mL, and then adjust the volume with water as needed to reach the final desired volume of 20 mL.
What Is The Net Ionic Equation For K2Co3?
The net ionic equation for K2CO3 is: 2K+ (aq) + CO3^2- (aq) → K2CO3 (s) This equation shows the dissociation of potassium ions and carbonate ions in aqueous solution to form solid potassium carbonate.
What is the correct formula for potassium carbonate?
the formula of potassium carbonate is k2co3 because the valency of potassium (k1+) valency of carbonate is (co32-) interchange the valencies and don't put the signs then it will become (k2co3) so the formulae of potassium carbonate is k2co3
Is K2CO3 basic or acidic?
K2CO3, potassium carbonate, is a salt that is basic in nature. It forms a basic solution when dissolved in water because it releases hydroxide ions which can accept protons to form water.
What is the balanced equation for the reaction that occurs when a student in a lab adds 150 ml of 1.00m AgNO3 solution to 100 ml of 1.00m K2CO3 solution.?
2AgNO3 + K2CO3 >> Ag2CO3 + 2KNO3 ( much more could be done with those numbers, but you did not ask for that ) ( Plus, I am not sure if Silver carbonate percipitates out of solution, so all those species could be dissasociated )
What is equation for rxn of benzoic acid with K2CO3?
K2CO3 + 2 benzoic acid -> 2 potassium benzoate + H2CO3
