![\Delta H=\sum [n\times \Delta H_f(product)]-\sum [n\times \Delta H_f(reactant)]](/tpl/images/1107/8427/76c37.png)
![\Delta H=[(n_{CO_2}\times \Delta H_{CO_2})+(n_{H_2O}\times \Delta H_{H_2O})]-[(n_{O_2}\times \Delta H_{O_2})+(n_{CH_4}\times \Delta H_{CH_4})]](/tpl/images/1107/8427/ce6cc.png)
![\Delta H=[(1\times -394)+(2\times -242]-[(2\times 0)+(1\times -75)]](/tpl/images/1107/8427/96065.png)
Chemistry question on enthalpy HELP
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Abeaker with 2.00×102 ml of an acetic acid buffer with a ph of 5.000 is sitting on a benchtop. the total molarity of acid and conjugate base in this buffer is 0.100 m. a student adds 4.70 ml of a 0.360 m hcl solution to the beaker. how much will the ph change? the pka of acetic acid is 4.740.
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