They both have the same concentration, but NaOH (Sodium Hydroxide) is more basic than NH4OH (Ammonium Hydroxide), because it breaks apart in H2O more easily. The OH-'s on both of them are technically the same, but the one in NaOH will break off more easily in water than that in NH4OH. Thus, NaOH is a stronger base and a stronger electrolyte.
Molar concentration in both base solutions NH3 and NaOH is assumed to be (equal) 0.1 mol Base/LWeak base like ammonia (NH3) with pKb = 9.2 and concentration (assumed) Cb = 0.1 (mol/L)pOH = 0.5*[pKb + pCb] = 0.5*[9.2 + 1.0] = 5.1 , hence [OH-] = 7.9*10-6pH = 14 - pOH = 8.9 hence [H+]= 1.3*10-9Strong base hydroxide (like from NaOH) with concentration (equally assumed) Cb = 0.1 (mol/L)pOH = 1.0 because [OH-] = 0.1pH = 13.0 hence [H+]= 1.0*10-13
Household ammonia has 10 times higher H+ concentration
Both would react with NaOH but one would react more readily.
In pure water, at standard conditions, the number of hydrogen ions (H⁺) is equal to the number of hydroxide ions (OH⁻). This balance occurs due to the self-ionization of water molecules: H 2 O ⇌ H OH − H 2 O⇌H +OH − For every water molecule that dissociates, one hydrogen ion (H⁺) and one hydroxide ion (OH⁻) are produced. The concentration of hydrogen ions (H⁺) is often denoted as [H⁺], and the concentration of hydroxide ions (OH⁻) is denoted as [OH⁻]. In neutral water (pH 7), these concentrations are equal: [H+]=[H−]=10−7 mol/L [H+ ]=[OH− ]=10−7 mol/L This balance ensures that the solution remains neutral. However, in acidic solutions, the concentration of hydrogen ions (H⁺) is higher than that of hydroxide ions (OH⁻), while in basic solutions, the concentration of hydroxide ions (OH⁻) is higher than that of hydrogen ions (H⁺). The product of the hydrogen ion concentration and the hydroxide ion concentration is always 10−14 mol 2 / L210−14 mol2 /L2 at 25°C, known as the ion product of water.
The OH concentration in a 4.0 x 10^4 M solution of Ca(OH)2 can be determined by dividing the concentration of Ca(OH)2 by its stoichiometric coefficient, which is 2. Thus, the OH concentration is 2.0 x 10^4 M.
Molar concentration in both base solutions NH3 and NaOH is assumed to be (equal) 0.1 mol Base/LWeak base like ammonia (NH3) with pKb = 9.2 and concentration (assumed) Cb = 0.1 (mol/L)pOH = 0.5*[pKb + pCb] = 0.5*[9.2 + 1.0] = 5.1 , hence [OH-] = 7.9*10-6pH = 14 - pOH = 8.9 hence [H+]= 1.3*10-9Strong base hydroxide (like from NaOH) with concentration (equally assumed) Cb = 0.1 (mol/L)pOH = 1.0 because [OH-] = 0.1pH = 13.0 hence [H+]= 1.0*10-13
To measure concentration, you compare the amount of the solute to the total amount of the solution.
Household ammonia has 10 times higher H+ concentration
Acid and Bases are different by its concentration of Hydrogen and Hydroxide. Acid is any compound that forms H+ ions in solution and base is a compound that forms OH- ions in solution. But Both are compounds forming a type of ion in a solution.
Both would react with NaOH but one would react more readily.
pH depends on concentration. However, the best way to compare bases (and acids) is to use the pKb value; the pKb of barium hydroxide is around -2, which makes it extremely basic.
There are a few different ways you could calculate the concentration of a salt solution with known conductivity. You could compare this amount of salt with pure water for example and take notes on the differences.
In pure water, at standard conditions, the number of hydrogen ions (H⁺) is equal to the number of hydroxide ions (OH⁻). This balance occurs due to the self-ionization of water molecules: H 2 O ⇌ H OH − H 2 O⇌H +OH − For every water molecule that dissociates, one hydrogen ion (H⁺) and one hydroxide ion (OH⁻) are produced. The concentration of hydrogen ions (H⁺) is often denoted as [H⁺], and the concentration of hydroxide ions (OH⁻) is denoted as [OH⁻]. In neutral water (pH 7), these concentrations are equal: [H+]=[H−]=10−7 mol/L [H+ ]=[OH− ]=10−7 mol/L This balance ensures that the solution remains neutral. However, in acidic solutions, the concentration of hydrogen ions (H⁺) is higher than that of hydroxide ions (OH⁻), while in basic solutions, the concentration of hydroxide ions (OH⁻) is higher than that of hydrogen ions (H⁺). The product of the hydrogen ion concentration and the hydroxide ion concentration is always 10−14 mol 2 / L210−14 mol2 /L2 at 25°C, known as the ion product of water.
when external environment has more water or diluted solution compare to the cell concentration, it is designated as hypotonic environment....
its different
The OH concentration in a 4.0 x 10^4 M solution of Ca(OH)2 can be determined by dividing the concentration of Ca(OH)2 by its stoichiometric coefficient, which is 2. Thus, the OH concentration is 2.0 x 10^4 M.
Hypertonic solution is the solution which contain more solute in it as compare to the cell internal solution now as the law of diffusion the solvent moves from low concentration of solute to high conc of solute so the solvent move out from the cell to the solution and cell ultimately will shrink