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What is the pH of 0.10 M HBr?
The pH of 0.10 M HBr is approximately 1.0. HBr is a strong acid that completely dissociates in water to produce H+ ions, leading to a low pH value.
What is the Ph of a 0.0030 M HBr solution in water?
The pH of a 0.0030 M HBr solution in water will be acidic due to the presence of HBr which is a strong acid. To calculate the pH, you can use the formula pH = -log[H+]. Since HBr ionizes completely in water to form H+ ions, the concentration of H+ ions in this solution would be 0.0030 M. Plugging this into the formula, you get pH = -log(0.0030) = 2.52. So, the pH of the solution is 2.52.
What is the pH of HBr in Bromine water?
HBr in water will dissociate to form hydronium ions (H3O+) and bromide ions (Br-). The presence of water will increase the acidity, resulting in a pH of less than 7 for this solution. The exact pH would depend on the concentration of the HBr solution.
A 25.00 mL sample of HBr is titrated with 0.150 M standardized sodium hydoxide solution the endpoint was reached when 18.80 mL of titrant had been added calculate the molar concentration of the HBr?
Using the balanced chemical equation for the reaction between HBr and NaOH (1:1 ratio), we can determine the moles of NaOH used. From the volume of NaOH used, we can then calculate the moles of HBr present in the sample. Finally, dividing moles of HBr by the initial volume of the sample (in liters) gives the molar concentration of HBr.
A solution of HBr has H 2.1 x 10-6 What is the pH of this solution?
By definition pH = -log[H+], so pH = -log(4.9*10-4) = 3.31Only at 25oC: pOH = 14.00 - pH, so 14.00 - 3.31 = 10.69 = pOH
What is the pH of 0.10 M HBr?
The pH of 0.10 M HBr is approximately 1.0. HBr is a strong acid that completely dissociates in water to produce H+ ions, leading to a low pH value.
What is the Ph of a 0.0030 M HBr solution in water?
The pH of a 0.0030 M HBr solution in water will be acidic due to the presence of HBr which is a strong acid. To calculate the pH, you can use the formula pH = -log[H+]. Since HBr ionizes completely in water to form H+ ions, the concentration of H+ ions in this solution would be 0.0030 M. Plugging this into the formula, you get pH = -log(0.0030) = 2.52. So, the pH of the solution is 2.52.
How do you determine the pH of a solution of 1.5 m of HBr?
pH=-log[H+] pH-log(1.2x10^-3) pH=2.92 since the the pH plus the pOH is always equal 14 14-2.92=11.08 so the pOH is 11.08
What is the pH of HBr in Bromine water?
HBr in water will dissociate to form hydronium ions (H3O+) and bromide ions (Br-). The presence of water will increase the acidity, resulting in a pH of less than 7 for this solution. The exact pH would depend on the concentration of the HBr solution.
A 25.00 mL sample of HBr is titrated with 0.150 M standardized sodium hydoxide solution the endpoint was reached when 18.80 mL of titrant had been added calculate the molar concentration of the HBr?
Using the balanced chemical equation for the reaction between HBr and NaOH (1:1 ratio), we can determine the moles of NaOH used. From the volume of NaOH used, we can then calculate the moles of HBr present in the sample. Finally, dividing moles of HBr by the initial volume of the sample (in liters) gives the molar concentration of HBr.
A solution of HBr has H 2.1 x 10-6 What is the pH of this solution?
By definition pH = -log[H+], so pH = -log(4.9*10-4) = 3.31Only at 25oC: pOH = 14.00 - pH, so 14.00 - 3.31 = 10.69 = pOH
What is the concentration of a HBr if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
To find the concentration of HBr, you first need to determine the number of moles of KOH that react with the HBr. This can be done using the volume and concentration of KOH solution. Then, using the stoichiometry of the neutralization reaction between HBr and KOH, you can find the number of moles of HBr present in the sample. Finally, divide the moles of HBr by the volume of the sample (12.0 mL) to obtain the concentration of HBr.
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.
A solution of HBr has H plus equals 2.1 x 10-6 What is the pH of this solution?
1.70
How many grams in 4.23 m mol of HBr?
The answer is 0,3422 grams.
A 76.0ml volume of 0.25m HBr is titrated with 0.50m KOH calculate the pH after addition of 38.0ml of KOH?
To calculate the pH after the addition of KOH, we need to determine the limiting reactant first. The limiting reactant will be the one that is completely consumed, in this case, HBr. The moles of HBr initially present can be calculated and then subtract the moles of KOH added to find the remaining HBr moles. Finally, calculate the concentration of HBr and find the pH using the concentration and dissociation constant of the acid.
Chemical Reaction between bromine and water?
When bromine reacts with water, it forms hydrobromic acid (HBr) and hypobromous acid (HOBr). The overall reaction can be represented as: Br2 + H2O → HBr + HOBr. This reaction is reversible and depends on the pH and conditions of the solution.
