7 - (-5) = 7 + 5 = 12 Taking away a negative number is defined as adding its absolute value.
If you subtract 4x on each side, you get 5 = -1, which is false. Note that this doesn't depend on the value of x, so this is false for any value of x.
The face value of 3 is 3: the value of 3 is 3000The face value of 5 is 5: the value of 5 is 500The face value of 3 is 3: the value of 3 is 3000The face value of 5 is 5: the value of 5 is 500The face value of 3 is 3: the value of 3 is 3000The face value of 5 is 5: the value of 5 is 500The face value of 3 is 3: the value of 3 is 3000The face value of 5 is 5: the value of 5 is 500
The sign of the sum will be the same as the number with the greatest absolute value. -9 + 4 = -5 -4 + 9 = 5
Absolute value of -5 is 5.
The pH value of potassium sulfate, K2SO4, is neutral, around 7. This is because potassium sulfate dissociates in water to release potassium ions (K+) and sulfate ions (SO4^2-) which do not significantly affect the pH of the solution.
The Ka for acetic acid (CH3COOH) is approximately 1.8 x 10^-5. This value represents the acid dissociation constant for acetic acid, indicating its strength as a weak acid. An acid with a higher Ka value will dissociate more readily in solution.
Knowing the pKa of an acid-base indicator allows us to determine the pH range over which the indicator changes color, making it useful for determining the endpoint of a titration. This information helps in selecting the appropriate indicator for a specific titration and ensures accurate results.
the organic compound three kind normal, acid and basic compound for acid compound the pKa from 3 to 5, normal pKa around 7 and basic compound more than 7 also you can know the kind of organic compound from structure that you can see acidic or basic grope like carboxylic acid or amine.
Cholic acid is a bile acid, a white crystalline substance insoluble in water, with a pKa of about 5.5. Urea is an organic compound with the chemical formula (NH2)2CO often found in the urine of animals, with a pKa of about 0.18.
To determine at which pH a drug will be 99.9% ionized, we need to consider the Henderson-Hasselbalch equation. The pH at which a drug is 99.9% ionized can be estimated by finding the pH value that is one unit above the pKa of the drug. Therefore, in this case, the drug will be 99.9% ionized at a pH of 6.
Of course the first 5 from right. 0.55 = 0.50 + 0.05, according the first 5 from right has a value of 0.05 while the first 5 from left has the value 0.50 which is ten times the other right 5.
The Ka value for ammonium nitrate is zero because it does not undergo significant dissociation into ions in water. Ammonium nitrate is a strong electrolyte and dissociates into ammonium and nitrate ions completely in water.
The pH after mixing two buffers can be calculated using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]), where [A-] is the concentration of conjugate base and [HA] is the concentration of the weak acid. Given pH of 4 and 6, the pKa can be determined and used in the equation to find the final pH value after mixing.
The dissociation constant, or pKa, of adipic acid is around 4.4. This means that adipic acid is a weak acid that partially dissociates in water to release hydrogen ions. The pKa value indicates the extent of ionization at a given pH.
7 - (-5) = 7 + 5 = 12 Taking away a negative number is defined as adding its absolute value.
Negative, because 5 is an odd number