you have to learn chemistry
Find moles HCl. 5 g HCl (1 mole HCl/36.450 grams) = 0.1372 moles HCl Now, Molarity = moles of solute/Liters of solution Molarity = 0.1372 moles HCl/1 liter = 0.1372 M HCl Then. -log(0.1372 M HCl) = 0.9 pH ( you might call it 1, but pH can be off the scale ) -----------
Molarity is the concentration of a solution, defined as moles per unit volume. Where, Molarity = moles / volume In this case the molarity of the HCl solution is 0.03 M The pH of this is calculated by the equation below pH = - log [H+] Where [H+] is the concentration of hydrogen ions/ protons present in the solution. As HCl only contains one hydrogen ion per molecule then the concentation of [H+] is 0.03 M Then the equation can be calculated (the minus sign is very important!) pH = - log 0.03 pH = 1.52 To summarise, Molarity of 0.03 M HCl solution is 0.03 M pH of 0.03 M HCl solution is 1.52
100 Liters? I will assume as much. Molarity = moles of solute/Liters of solution Molarity = 0.10 mole HCl/100.0 Liters = 0.001 M HCl -------------------------now, to find pH - log(0.001 M HCl) = 3 pH -----------------so, your acid is of 3 pH, which is to be expected at the volume od solution
HCl is a strong acid, so we assume that it completely breaks up into ions in solution. HCl ----> H+ & Cl- if we have 0.01m of HCl, it will give 0.01m of H+ and 0.01m Cl- pH = -log [H+] pH = -log 0.01 pH = 2
It solely depends on H+ concentration: each HCl gives one H+ , to calculate use pH = -log[H+] So, at [HCl]=1.0 >> pH= 0.0 at [HCl]=0.5 >> pH= 0.7 at [HCl]=0.1 >> pH= 1.0 at [HCl]=1.0*10-5 >> pH= 5.0 but don't ever use this simplified 'acid pH' calculus method when the answer comes close to (or exceeds) 6.5, 7 or 8 etc.
Find moles HCl. 5 g HCl (1 mole HCl/36.450 grams) = 0.1372 moles HCl Now, Molarity = moles of solute/Liters of solution Molarity = 0.1372 moles HCl/1 liter = 0.1372 M HCl Then. -log(0.1372 M HCl) = 0.9 pH ( you might call it 1, but pH can be off the scale ) -----------
Molarity is the concentration of a solution, defined as moles per unit volume. Where, Molarity = moles / volume In this case the molarity of the HCl solution is 0.03 M The pH of this is calculated by the equation below pH = - log [H+] Where [H+] is the concentration of hydrogen ions/ protons present in the solution. As HCl only contains one hydrogen ion per molecule then the concentation of [H+] is 0.03 M Then the equation can be calculated (the minus sign is very important!) pH = - log 0.03 pH = 1.52 To summarise, Molarity of 0.03 M HCl solution is 0.03 M pH of 0.03 M HCl solution is 1.52
100 Liters? I will assume as much. Molarity = moles of solute/Liters of solution Molarity = 0.10 mole HCl/100.0 Liters = 0.001 M HCl -------------------------now, to find pH - log(0.001 M HCl) = 3 pH -----------------so, your acid is of 3 pH, which is to be expected at the volume od solution
HCl is a strong acid, so we assume that it completely breaks up into ions in solution. HCl ----> H+ & Cl- if we have 0.01m of HCl, it will give 0.01m of H+ and 0.01m Cl- pH = -log [H+] pH = -log 0.01 pH = 2
I think it'd be pH 7. Same amount of both, providing they are the same molarity!
It solely depends on H+ concentration: each HCl gives one H+ , to calculate use pH = -log[H+] So, at [HCl]=1.0 >> pH= 0.0 at [HCl]=0.5 >> pH= 0.7 at [HCl]=0.1 >> pH= 1.0 at [HCl]=1.0*10-5 >> pH= 5.0 but don't ever use this simplified 'acid pH' calculus method when the answer comes close to (or exceeds) 6.5, 7 or 8 etc.
The answer depends on several unspecified variables, most importantly the final molarity of the solution, which depends on the final volume. You can calculate the value yourself using the formula: pH = -log[H+] where [H+] is the final concentration of H+ ions in solution. For HCl, [H+] is equal to molarity. So, for example, if you add 50.0 ml of 1.0M HCl to 950 ml of deionized water, your final concentation is: (50.0 ml/1000 ml) * (1.0M) = 0.05M Therefore: pH = -log[0.05] = 1.3
pH = -log10[H+], where [H+] is the hydrogen ion concentration. So, in this case, pH = -log10[1], yielding pH = 0.
HCl is a strong acid and dissociates completely. Therefore it can be found using the equation: ph= -log [H+]
- log(0.25 M HCl) = 0.6 pH ------------
- log(0.00450 M HCl)= 2.3 pH=======
The pH scale is a convenient method for expressing the hydronium ion concentration of a solution. pH = log(1/[H+]) = -log [H+]. [H+] is the hydronium ion concentration in M (molarity), which is the number of moles of solute per liter of solution.