A quantity of ethyl acetate is mixed with an excess of sodium hydroxide at ${25}^{°}$C. $100$ c.c. of the mixture is immediately titrated against $0.05 \mathrm{N}$ Hydrochloric acid, of which $75$ c.c were required for neutralisation. After $30$ minutes, $50$ c.c. of the mixture required, similarly, $25$ c.c. of the acid. When the original reaction of ester was complete, $25$ c.c. of the mixture required $6.25$ c.c. of the acid. Calculate the second order velocity constant (in $\mathrm{mol}/\mathrm{A}/\min$) (at time $=0$ ) of the reaction, using concentration in moles per litre and time in minutes. Reaction is first order each w.r.t. $\mathrm{NaOH}$ and ester. Indicator chosen for above titration is such that, it gives end point when only hydrochloric acid reacts with $(\log 2=0.30$, $\log 3 = 0.48$, $\log 10 = 2.3)$ (Give your Answer after multiplying with a factor of $10$ and excluding the decimal places)