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What is the chemical equation for potassium iodide?
The chemical formula for potassium iodide is KI. When dissolved in water, it dissociates into potassium ions (K+) and iodide ions (I-). The equation for this dissociation is written as: KI → K+ + I-.
When the ionic compound KI is dissolved in water?
When the ionic compound KI (potassium iodide) is dissolved in water, it dissociates into its constituent ions: K+ and I-. The solution will conduct electricity due to the presence of mobile ions and will likely exhibit properties such as color changes or precipitation reactions, depending on the specific reaction involved.
Is KI in H20 an electrolyte?
Yes. KI is an ionic compound and dissociates completely to K+ and I- ions making it a strong electrolyte.
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 495 mL solution containing 21.1 g of potassium iodide?
We have 495 ml, but we need to convert this to 1000, so we divide by 495 and multiply by 1000. We also do this to 21.1g. 21.1/495*100 is 42.626g. KI's molecular weight is 166g/mol. 42.626/166 is 0.2568 molar.
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 820mL of Kl solution that contains 36.52g of Kl?
To find the molarity (M) of the KI solution, first convert grams of KI to moles using its molar mass (KI's molar mass is approximately 166 g/mol). Moles of KI = 36.52 g / 166 g/mol ≈ 0.220 moles. Then, convert the volume from mL to liters: 820 mL = 0.820 L. Finally, calculate the molarity: M = moles/volume = 0.220 moles / 0.820 L ≈ 0.268 M. Thus, the molarity of the KI solution is approximately 0.268 M.
How many grams of KI are required to prepare 500ml of 0.04 M KI?
To calculate the grams of KI required, use the formula: grams = molarity (M) × volume (L) × molar mass (g/mol). The molarity is 0.04 M and the volume is 0.5 L (500 ml). The molar mass of KI is approximately 166 g/mol. Therefore, grams of KI required = 0.04 M × 0.5 L × 166 g/mol = 3.32 grams.
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 is the molarity of 820 ml of Kl solution that contains 36.52 g of Kl?
To find the molarity (M) of the solution, first calculate the number of moles of KI. The molar mass of KI is approximately 166 g/mol (39 g/mol for K and 127 g/mol for I). So, the number of moles in 36.52 g of KI is 36.52 g ÷ 166 g/mol ≈ 0.22 moles. The volume of the solution in liters is 820 ml ÷ 1000 = 0.82 L. Therefore, the molarity is M = moles/volume = 0.22 moles / 0.82 L ≈ 0.27 M.
What is the molarity of 820 mL of KI solution that contains 36.52 g of KI?
To find the molarity, first calculate the number of moles of KI using its molar mass (KI has a molar mass of approximately 166 g/mol). The number of moles is calculated as follows: [ \text{Moles of KI} = \frac{36.52 \text{ g}}{166 \text{ g/mol}} \approx 0.22 \text{ moles} ] Next, convert the volume from mL to liters: ( 820 \text{ mL} = 0.820 \text{ L} ). Finally, calculate the molarity (M): [ \text{Molarity} = \frac{\text{moles of solute}}{\text{liters of solution}} = \frac{0.22 \text{ moles}}{0.820 \text{ L}} \approx 0.27 \text{ M} ] Thus, the molarity of the KI solution is approximately 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.
What is the maximum amount of KI that can be dissolved in 50 mL of water at 30 C?
The solubility of KI at 30°C is about 50g/100mL of water. Therefore, in 50mL of water, you can dissolve a maximum of 25g of KI at 30°C.
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
Is ki aqueous?
No, ki is not aqueous. Aqueous refers to a substance that is dissolved in water. Ki is a term in Japanese culture that represents life energy or spirit in a more abstract sense.
What is the chemical equation for potassium iodide?
The chemical formula for potassium iodide is KI. When dissolved in water, it dissociates into potassium ions (K+) and iodide ions (I-). The equation for this dissociation is written as: KI → K+ + I-.
When the ionic compound KI is dissolved in water?
When the ionic compound KI (potassium iodide) is dissolved in water, it dissociates into its constituent ions: K+ and I-. The solution will conduct electricity due to the presence of mobile ions and will likely exhibit properties such as color changes or precipitation reactions, depending on the specific reaction involved.
