Step 1:If asked for the conjugate acid,attachanHto the given formula andincreaseits charge by one. If asked for the conjugate base,removeanHanddecreaseits charge by one. Bronsted-Lowry Acids and Bases:When the Bronsted-Lowry concept of acids and bases was introduced in 1923, it differed from...
In the Bronsted-Lowry formulation of acids and bases, an acid is a compound that releases a proton in solution, while a base is a compound that accepts a proton. When a Bronsted acid dissolves in a solvent, it produces a conjugate base, while at the same time the solvent acts as a ba...
Identify its conjugate acid or base. Is OH- an acid or a base? Identify its conjugate acid or base. How do you find the bronsted acid in a reaction or how do you determine which one is the proton donors? Identify the Bronsted acids and bases in the following equation. H S O ...
how can I determine the strongest base according to the Bronsted-Lowry theory? NO3, F, I, ClMy reasoning: HNO3 is a strong acid (by using the table of strong acids), so NO3 is its weak conjugate base; the same is true about HCl and HI; HF is a weak acid, so F is its strong...
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What determines whether or not an acid is strong? What are some of the strong acids? What determines whether or not a base is strong? What are some of the strong bases? Is the conjugate base of a strong acid itself strong? Explain why or why not. ...
Read the problem, and write down the information that is given. In a problem that involves calculating the Kb from the Ka, you are usually given the Ka and the Kw. For example, you may be asked to calculate the Kb of the chloride ion. The given Ka of the conjugate acid of the chlo...
Decide on the pH for your buffer. This pH should be within one pH unit from the pKa of the acid/conjugate base. So, you can prepare a buffer at pH 2 or pH 7, for example, but pH 9 would be pushing it. Use theHenderson-Hasselbachequation to calculate how much acid and base you ...
To calculate the pH of an acid buffer, the Henderson-Hasselbalch equation is used, which is pH = pKa + log(acid/base). The acid's concentration is on top of the fraction, and the conjugate base's is on the bottom. What is the pH of a buffer? The pH of a solution, buffer or ...
Chemically, buffers consist of a weak acid and its conjugate base or a weak base and its conjugate acid. When an acidic solution is added to a buffer, the weak acid reacts with the excess H+ ions to form more of the conjugate base, thus decreasing the concentration of H+ ions to ...