We use this law to determine the pH value of a buffer solution considering the acid dissociation constant and concentrations of acid and base. We define {eq}pK_a {/eq} using the acid dissociation constant {eq}K_a {/eq} considering the below expressio...
Ammonium {eq}NH_4+{/eq} Solving for acid dissociation constant {eq}K_a{/eq} of Ammonium...
属于氧化还原反应的是( ) A.CaCO3=+CO2↑ B.NH3+HCl=NH4Cl C.NaOH+HCl=NaCl+H2O D.Zn+H2SO4(稀)=ZnSO4+H2↑ 查看完整题目与答案 高中化学>氧化还原反应的本质和特征考试题目 计算题(1)(1- 1 6 + 3 4 )×(-48)(2)(-1)10×2+(-2)3÷4(3) 2 3 - 1 8 -(- 1 3 )+(- 3 8 ...
They form a dissociation equilibrium according to a Ka value, which determines the solution's hydrogen ion molarity and ultimately its pH Answer and Explanation: The question describes the creation of a buffer solution composed of a weak...
Not a buffer Buffering Solution: A buffering solution maintains a constant pH by eliminating the effects of a change in the concentration of H+ ions. This is achieved through two equilibrium reactions. Answer and Explanation:1 Buffers require a weak...
A buffer is 0.10 M in NH3 and 0.10 M in NH4Cl. What is the pH of the solution after the addition of 10.0 mL of 0.20 M of HCl to 100.0 mL of the buffer? What volume of 0.200 M HCl must be added to 250.0 mL of 0....
Suppose you add 10 mL of 0.10 M sodium hydroxide to 0.1 L of a buffer solution (60 mL of 0.1 M NH3 and 40 mL of 0.100 M NH4Cl). What is the pH? The Ka of NH3 is 1.8 x 10^-5. A buffer was made with 100 ml o...