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How many milliliters of 6.0 M NaOH must be used to prepare 1.0 liter of 0.10 M solution?
To prepare a 0.10 M NaOH solution, you need to dilute the 6.0 M solution. You can use the formula: M1V1 = M2V2 where M1 = 6.0 M, V1 is the volume of 6.0 M NaOH needed, M2 = 0.10 M, and V2 = 1000 mL (1.0 L). By substituting the values into the formula, you can calculate the volume of the 6.0 M NaOH needed to prepare the 0.10 M solution.
Which 1.0 M acid solution has the largest concentration of hydronium H3O?
A 1.0 M hydrochloric acid (HCl) solution would have the largest concentration of hydronium ions (H3O+) since each mole of HCl dissociates completely to form one mole of H3O+. This means that the concentration of H3O+ ions in a 1.0 M HCl solution would also be 1.0 M.
What is the H3O in a solution of OH- 1x10-12M?
- log(1 X 10 -12 M) = 12 pH -----------------------very little room for H3O
What is the molarity of HNO3 if 20.0 ml of the solution is needed to exactly neutralize 10.0 ml of a 1.67 M NaOH solution?
The reaction between HNO3 and NaOH is a 1:1 molar ratio. This means that the moles of HNO3 required to neutralize the NaOH is the same as the moles of NaOH. Given that 20.0 ml of HNO3 is needed to neutralize 10.0 ml of a 1.67 M NaOH solution, the molarity of the HNO3 solution is twice the molarity of the NaOH solution, which is 3.34 M.
What is the pH of a solution with a H3O of 7.9x10-11 M?
The pH of a solution with a H3O+ concentration of 7.9x10-11 M is approximately 10.1. This is because pH is calculated as -log[H3O+], so -log(7.9x10-11) ≈ 10.1.
How many grams of NaOH are in 750 ml 0.600 M NaOH solution?
This solution contain 26,3 g NaOH.
How many milliliters of 6.0 M NaOH must be used to prepare 1.0 liter of 0.10 M solution?
To prepare a 0.10 M NaOH solution, you need to dilute the 6.0 M solution. You can use the formula: M1V1 = M2V2 where M1 = 6.0 M, V1 is the volume of 6.0 M NaOH needed, M2 = 0.10 M, and V2 = 1000 mL (1.0 L). By substituting the values into the formula, you can calculate the volume of the 6.0 M NaOH needed to prepare the 0.10 M solution.
A 20.0ml sample of 0.800 m Hbr solution is titrated with 0.800 m NaOH solution calculate the pH of the solution after these volumes of base are added 12.5 ml 18.7 ml 20.0 ml 29.5 ml and 34.2?
To calculate the pH after each volume of NaOH is added, you need to determine the moles of HBr initially, moles of NaOH added, and then use these values to calculate the final concentration of H3O+ ions in the solution. From there, you can calculate the pH using the equation pH = -log[H3O+]. Repeat these calculations for each volume of NaOH added to find the pH at 12.5 ml, 18.7 ml, 20.0 ml, 29.5 ml, and 34.2 ml.
Which 1.0 M acid solution has the largest concentration of hydronium H3O?
A 1.0 M hydrochloric acid (HCl) solution would have the largest concentration of hydronium ions (H3O+) since each mole of HCl dissociates completely to form one mole of H3O+. This means that the concentration of H3O+ ions in a 1.0 M HCl solution would also be 1.0 M.
What is the molarity of HNO3 if 20.0 ml of the solution is needed to exactly neutralize 10.0 ml of a 1.67 M NaOH solution?
The reaction between HNO3 and NaOH is a 1:1 molar ratio. This means that the moles of HNO3 required to neutralize the NaOH is the same as the moles of NaOH. Given that 20.0 ml of HNO3 is needed to neutralize 10.0 ml of a 1.67 M NaOH solution, the molarity of the HNO3 solution is twice the molarity of the NaOH solution, which is 3.34 M.
What is the H3O in a solution of OH- 1x10-12M?
- log(1 X 10 -12 M) = 12 pH -----------------------very little room for H3O
What is the pH of a solution with a H3O of 7.9x10-11 M?
The pH of a solution with a H3O+ concentration of 7.9x10-11 M is approximately 10.1. This is because pH is calculated as -log[H3O+], so -log(7.9x10-11) ≈ 10.1.
What is the pH of a 0.33 M solution of NaOH?
The pH of a 0.33 M solution of NaOH is approximately 13.5. This is because NaOH is a strong base that dissociates completely in water to give hydroxide ions, which results in a highly alkaline solution.
What is the pH of a cleaning solution with a H3O 7.4 10-9 M H3O?
By definition: pH = -log[H3O+]So pH = -log(7.4*10-9) = 8.13
What is the pH of a solution with 0001 M H3O?
3. since the [H+]=0.001 M then pH= -log[H+] -log(0.001)=3 pH=3.
How much NaOH is in 3.8 L of a 0.53 M NaOH solution?
Molarity = moles of solute/volume of solution 0.53 M NaOH = moles NaOH/3.8 Liters = 2.014 moles, or about 80 grams
What is the pH of a 10-4 M naoh solution?
-log(10^-4 M NaOH) = 4 14 - 4 = 10 pH NaOH -----------------------
