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Calculate the mass of ki in grams required to prepare 5.00 102 ml of a 2.80 m solution?
To calculate the mass of KI needed for a 2.80 m solution, we first need to know the molality (m) and the volume of the solution. The molality is defined as moles of solute per kilogram of solvent. For a 2.80 m solution, we have 2.80 moles of KI per kg of solvent. Given the volume of 5.00 x 10² mL (or 0.500 kg of water, assuming the density of water is 1 g/mL), we can use the formula: Mass of KI = moles of KI × molar mass of KI. Calculating, we find that 2.80 moles of KI correspond to about 2.80 × 166 g/mol (molar mass of KI) = 464.8 g of KI. Thus, you need approximately 464.8 grams of KI.
What is the molarity of 67.94 mL aqueous solution containing 2.822 g of KI?
Molarity = moles of solute/Liters of solution. get moles KI 2.822 grams KI (1 mole KI/166 grams) = 0.017 moles KI ( 67.94 ml = 0.06794 Liters ) Molarity = 0.017 moles KI/0.06794 Liters = 0.2502 M KI
What is the molarity of 820 ml of KI solution tat contains 36.52g of kI?
To find the molarity (M) of the KI solution, first calculate the number of moles of KI using its molar mass. The molar mass of KI (potassium iodide) is approximately 166 g/mol. Thus, moles of KI = 36.52 g / 166 g/mol ≈ 0.22 moles. Since the solution volume is 820 ml (or 0.82 L), the molarity is M = moles/volume = 0.22 moles / 0.82 L ≈ 0.27 M.
What mass of KI is present in 276 mL of a 0.50 M solution?
To calculate the mass of KI in the solution, first calculate the number of moles of KI present using the formula moles = Molarity x Volume (in liters). Then, use the molar mass of KI (potassium iodide) to convert moles to grams. The molar mass of KI is 166 g/mol.
Is SnI4 soluble in KI solution?
Hi, having a solution of KI implies having H20 so tin iodide will hydrolyze forming the tin oxide and HI. Another interesting reaction is when you add KI (in solid phase) into tin iodide solution (dissolved in acetone). You will obtain a salt like this: K(SnI5) I hope I helped you. Note that this answer could be wrong, I'm currently a student of chemistry and I have a lot to learn yet.
To 225 mL of a 0.80M solution of KI a student adds enough water to make 1.0 L of a more dilute KI solution What is the molarity of the new solution?
0.18M
How do you prepare a 10 percent potassium iodide solution?
To prepare a 10% potassium iodide solution, dissolve 10 grams of potassium iodide in 90 ml of water. Don't forget to wear appropriate protective gear like gloves and goggles. Stir the mixture well until the potassium iodide is fully dissolved.
Calculate the mass of ki in grams required to prepare 5.00 102 ml of a 2.80 m solution?
To calculate the mass of KI needed for a 2.80 m solution, we first need to know the molality (m) and the volume of the solution. The molality is defined as moles of solute per kilogram of solvent. For a 2.80 m solution, we have 2.80 moles of KI per kg of solvent. Given the volume of 5.00 x 10² mL (or 0.500 kg of water, assuming the density of water is 1 g/mL), we can use the formula: Mass of KI = moles of KI × molar mass of KI. Calculating, we find that 2.80 moles of KI correspond to about 2.80 × 166 g/mol (molar mass of KI) = 464.8 g of KI. Thus, you need approximately 464.8 grams of KI.
How many grams of KI are in 25.0ml of a 3.0 (mv) KI solution?
55 ml of a 4.05 M solution of KI solution contains 55*4.05=222.75 millimoles. 20.5 ml of the diluted solution contains 3.8g of KI,so no.of moles of KI=3.8/(mol.wt of KI=165.9) is 22.9 millimoles. molarity of final diluted solution=22.9/20.5=1.117M since the no. of moles of KI present in initial and final solution are same. let.V(in ml) be the final volume of diluted solution. 222.75/V=1.117 V=199.41 ml final volume =199.41 ml
What is the molarity of 67.94 mL aqueous solution containing 2.822 g of KI?
Molarity = moles of solute/Liters of solution. get moles KI 2.822 grams KI (1 mole KI/166 grams) = 0.017 moles KI ( 67.94 ml = 0.06794 Liters ) Molarity = 0.017 moles KI/0.06794 Liters = 0.2502 M KI
How do you prepare iodine solution?
To prepare iodine solution, dissolve iodine crystals in a mixture of water and potassium iodide (KI). The ratio of iodine to KI will determine the concentration of the solution. The solution should be stored in a dark bottle to prevent degradation from light exposure.
Why is KI a neutral solution?
Potassium iodide (KI) is considered a neutral solution because it dissociates in water to form potassium ions (K^+) and iodide ions (I^-), which do not affect the pH of the solution. The ions from KI do not contribute to the acidity or basicity of the solution, meaning that KI does not alter the pH level significantly.
What is the molarity of 820 ml of KI solution tat contains 36.52g of kI?
To find the molarity (M) of the KI solution, first calculate the number of moles of KI using its molar mass. The molar mass of KI (potassium iodide) is approximately 166 g/mol. Thus, moles of KI = 36.52 g / 166 g/mol ≈ 0.22 moles. Since the solution volume is 820 ml (or 0.82 L), the molarity is M = moles/volume = 0.22 moles / 0.82 L ≈ 0.27 M.
What is the molarity of a solution prepared by dissolving 2.41 g of potassium iodide KI in 100 mL of water?
Find moles potassium iodide first.2.41 grams KI (1 mole KI/166 grams) = 0.01452 moles KIMolarity = moles of solute/Liters of solution ( 100 ml = 0.1 Liters )Molarity = 0.01452 moles KI/0.1 Liters= 0.145 M KI solution================
What mass of KI is present in 276 mL of a 0.50 M solution?
To calculate the mass of KI in the solution, first calculate the number of moles of KI present using the formula moles = Molarity x Volume (in liters). Then, use the molar mass of KI (potassium iodide) to convert moles to grams. The molar mass of KI is 166 g/mol.
What is the pH of KI?
KI (potassium iodide) is a salt that dissociates into K+ and I- ions in water. Both potassium ions and iodide ions are neutral and do not affect the pH of a solution. Therefore, the pH of a solution of KI would remain unchanged.
When was Inochi no Ki created?
Inochi no Ki was created on 2010-10-06.
