How do you calculate the pH of a 0.1 M HCl solution?
pH=−log[H+]=−log10−1=1. Was this answer helpful?
A 0.010 M solution of hydrochloric acid, HCl, has a molarity of 0.010 M. This means that [H+] = 1 x 10-2 M. The pH of this aqueous solution of H+ ions is pH = 2. You will notice that the pH number is just the positive exponent of 10 from the Molar concentration.
First we should know about the concentration of HCl solution or the molarity of the solution, then by applying the pH formula as pH=−log[H+], we can easily find the pH of the solution.
The pH of 0.01 M solution of acetic acid is 5.0.
An acid has a molarity of 0.01M means that the molar concentration of the acid is 0.01M. To put it very simply, let us consider that the molecular weight of the acid is X. Now, if X gm of the acid is added to a solvent to make a final solution of 1ltr, the solution will have a concentration of 1M.
Thus, $0.001{\text{ M}}$ solution of ${\text{HCl}}$ is 3. Thus, the correct option is (B) 3. Note: The concentration of hydrogen ion is known as the pH. The pH is calculated as the negative logarithm of the hydrogen ion concentration.
Hydrochloric acid, 0.01N standardized solution is used for volumetric analysis in laboratories. This Thermo Scientific Chemicals brand product was originally part of the Alfa Aesar product portfolio. Some documentation and label information may refer to the legacy brand.
sodium phosphate buffer, pH 7.0.
pH=−log10[H+]=−log10[0. 005×2]=−log10[0. 001]=2−log1=2. Was this answer helpful?
Solution : The diluted `HCI` is `0.1 M` do that `pH = 1.00`.
What is the pH of 0.01 M of NaOH solution?
If 0.01 mole of NaOH is added to 1 litre solution of a basic buffer having pH=8.7 initially, the pH changes to 9.
So, a 0.01M NaOH solution will have a pH of 12 .
Expert-Verified Answer
0.01M HCl means that 0.01 moles of HCl are present in 1000mL of solution. or 0.365 g HCl are present in 1000mL of solution.
The pH scale is a convenient way to represent the acidity or basicity of a solution. We can calculate the pH of a solution by taking the negative logarithm of the hydronium ion concentration, or pH = -log[H₃O⁺].
0.1M Hydrochloric Acid is often used for acid-base reactions, refinement, and pH control. This chemical is suitable for use in any educational or research laboratory that deals with organic chemistry or biochemistry. Bottle has safe handling and storage procedures printed directly on the bottle.
[H+] Concentration in 0.01 M HCl is 10−2 M because 0.01 M HCl have only H+.
| CAS | 7647-01-0,7732-18-5 |
|---|---|
| Physical Form | Liquid |
| Concentration or Composition (by Analyte or Components) | 0.5N (N/2) |
| Packaging | Poly Bottle |
| pH | 0.10 |
pH of 10−xM HCl is 6.9586.
You will need to know the molarity of the NaOH. Let's assume the solution is 0.1M. NaOH is a strong base, so this will produce 0.1mol/L of OH ions in solution. This will produce a pH of 13.
The pH of a 0.1 M solution of acid HA is 1.0.
What is the pH of a 12.0 m HCl solution?
All metal hydroxides are strong bases. The pH of a 12.0 M solution of HCl is −1.1.
Aqueous solution of HCl has the pH =4.
pH=0. 468.
The pH of 1 M hydrochloric acid is zero. The reason is that pH is defined as negative 1 times the log base 10 of [H+], or the proton concentration in moles per liter.
If 0.01 mole of NaOH is added to 1 litre solution of a basic buffer having pH=8.7 initially, the pH changes to 9.
The pH of 0.01 M solution of acetic acid is 5.0.
pH=−log10[H+]=−log10[0. 005×2]=−log10[0. 001]=2−log1=2.